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SOLUBILITIES 

OF 

INORGANIC  AND  ORGANIC 
SUBSTANCES 

A  HANDBOOK  OF  THE  MOST  RELIABLE 

QUANTITATIVE   SOLUBILITY 

DETERMINA  TIONS 


RECALCULATED   AND   COMPILED   BY 

ATHERTON  SEIDELL,  PH.D.  (J.H.U.) 

Chemist,    Division    of  Pharmacology,    Hygienic   Laboratory    of  the    U.  .S, 

Public  Health  and  Marine-Hospital  Service,    Washington,  D.  C. 

Formerly  Assistant  Chemist,  Bureau  of  Chemistry 

U.  S.  Department  of  Agriculture 


Second  Printing  with  Corrections 


NEW  YORK: 

D.   VAN    NOSTRAND    COMPANY 

LONDON : 

CROSBY    LOCKWOOD   &    SON, 

7  STATIONERS'  HALL  COURT,  LUDGATE  HILL 

1911 


m/ 

PHYSICS  D£PT» 


COPYRIGHT,  1907  AND  1911  BY 
D.  VAN   NOSTRAND   COMPANY 


Stanbope 


H        01  LSO  N       COM  PAHT 

BOSTON.        U.    S.    A. 


PREFACE 

DURING  the  years  which  have  elapsed  since  Professor  Arthur  M. 
Comey's  admirable  "Dictionary  of  Chemical  Solubilities"  went 
to  press  (March,  1894),  the  literature  upon  solubilities  has  grown 
to  such  an  extent  that  it  has  appeared  desirable  to  make  a  new 
compilation  of  it.  Soon  after  beginning  work  upon  this  volume  the 
author  realized  that  it  would  not  be  possible  to  prepare  a  com- 
pilation of  solubility  results  which  would  fulfill  completely  the 
various  requirements  of  theoretical,  technical,  analytical,  and 
other  classes  of  chemists,  and  he  has  therefore  endeavored  to  meet 
some  of  the  needs  of  all  chemists  rather  than  provide  information 
especially  arranged  for  any  particular  class. 

The  following  features  have  been  considered  of  chief  impor- 
tance in  preparing  the  present  compilation:  completeness  of  the 
data,  reliability  of  the  determinations,  uniformity  in  expression 
of  results,  convenience  of  arrangement  of  material,  and  the  index- 
ing of  the  cross-references  to  tables. 

The  material  has  been  collected  almost  entirely  from  the  origi- 
nal sources,  and  not  from  text-books  or  works  of  reference. 
The  plan  followed  has  been  to  search  diligently  the  tables  of  con- 
tents or  indices  of  twenty -five  of  the  principal  chemical  journals 
issued  since  1875,  and  to  consult  all  articles  in  these  as  well  as  in 
other  journals  to  which  references  could  be  obtained.  In  this 
connection,  however,  it  should  be  stated  that  indexed  references 
to  work  on  solubility  usually  appear  under  the  name  of  the  sub- 
stance employed,  and  not  under  the  heading  "solubility."  Fur- 
thermore, solubility  determinations  are  often  incidental  to  other 
investigations,  and  consequently  are  not  indicated  in  the  title 
of  the  article  or  included  in  the  index  of  the  journal.  Consid- 
ering these  difficulties  there  can  be  little  hope  of  making  such 
a  compilation  complete  in  every  detail,  and  in  the  present  case 
the  best  that  can  be  said  is  that  an  earnest  effort  has  been  made 
to  omit  nothing  of  importance.  This  has  been  done  not  only 
for  the  author's  personal  satisfaction  in  perfecting  the  work, 
but  also  to  give  the  reader  a  reasonable  assurance  that  the  ab- 
sence from  these  pages  of  results  upon  a  particular  substance  is 
good  evidence  that  such  determinations  of  satisfactory  reliability 

iii 

222563 


PREFACE 

are  not  readily  obtainable  from  the  usually  accessible  chemical 
journals. 

Although  at  the  time  Professor  Comey  compiled  his  book  it 
appeared  inadvisable  to  attempt,  in  the  majority  of  cases,  to 
select  the  most  reliable  determinations  of  the  solubility  of  the 
same  substance  reported  by  different  investigators,  the  present 
author  believes  that  this  can  now  be  done  with  advantage.  The 
selections  have  been  made  in  all  cases  by  calculating  the  avail- 
able determinations  to  a  common  basis  and  drawing  curves 
through  the  points  plotted  on  cross-section  paper.  A  comparison 
of  the  curves,  together  with  a  study  of  the  details  of  the  methods 
by  which  the  determinations  were  made  in  the  several  cases,  has 
usually  furnished  clear  evidence  for  a  reliable  selection.  For 
some  substances,  however,  this  plan  could  not  be  followed,  and 
it  has  therefore  been  necessary  to  present  two  or  more  sets  of 
disagreeing  results. 

In  many  instances  the  calculations  and  study  necessary  to 
ascertain  the  most  reliable  figures  have  required  much  labor, 
and  perhaps  in  some  cases  the  author  has  not  succeeded  in 
selecting  the  ones  nearest  the  truth;  but  it  is  believed  that  the 
economy  of  space  required  to  present  the  material,  and  the  saving 
of  the  time  of  the  reader  in  making  the  necessary  selections  him- 
self, will  far  overbalance  the  disadvantage  resulting  from  the 
accidental  inaccuracies  introduced  through  extended  computa- 
tions. 

An  additional  advantage  resulting  from  the  recalculation  of 
different  determinations  to  a  common  basis  is  the  increased 
uniformity  in  the  expression  of  results  throughout  the  volume. 
On  this  account  it  has  been  possible  to  give  the  solubility  of  most 
substances  for  regular  intervals  of  temperature  and  in  terms  of 
weight  of  dissolved  substance  per  given  weight  of  solvent  or  of 
solution. 

Quantitative  results  alone  have  been  included  in  this  com- 
pilation, since  it  is  assumed  that  qualitative  determinations,  if 
desired,  can  be  readily  made  by  simple  tests  in  the  laboratory, 
and  therefore  the  effort  necessary  to  collect  such  observations 
from  the  literature  is  out  of  proportion  to  the  value  of  the  inform- 
ation obtained. 

In  regard  to  the  names  and  formulas  of  the  compounds  in- 
cluded, the  author  wishes  to  say  that  they  are,  for  the  most  part, 
given  as  found  in  the  original  papers  from  which  they  were  taken ; 
and  in  some  cases  a  lack  of  uniformity  in  the  manner  of  their 

iv 


PREFACE 

expression  will  be  noted.  This  is  especially  true  of  the  molecules 
of  water  of  crystallization  in  the  formulas  given  in  connection 
with  the  guide  names  placed  in  heavy  type  at  the  head  of  the 
tables  for  all  substances  considered.  As  is  well  known,  many 
compounds,  besides  gaming  or  losing  water  in  air,  also  crystal- 
lize with  different  numbers  of  molecules  of  water  even  at  the 
ordinary  temperature,  and  it  was  therefore  thought  best  to  include 
such  information  at  the  proper  place  in  the  tables  under  the 
heading  "Solid  Phase"  rather  than  to  select  in  doubtful  cases 
the  number  of  molecules  of  water  which  the  particular  substance 
was  considered  to  carry  under  ordinary  conditions. 

Although  the  arrangement  of  the  material  is  alphabetical  accord- 
ing to  the  customary  English  names,  an  index  has  been  added 
which  also  provides  for  those  cases  where  there  appears  a  doubt 
as  to  which  name  is  preferable,  and  furnishes  cross-references  to 
those  tables  which  contain  results  upon  more  than  one  substance. 

A  glance  through  the  pages  of  this  book  will  show  the  incom- 
pleteness of  the  data  for  many  of  the  most  common  chemical 
compounds.  Furthermore  many  of  the  results  given  are  of 
doubtful  accuracy,  although  the  best  available.  It  is  hoped, 
therefore,  that  a  realization  of  the  present  incomplete  state  of  our 
information  concerning  solubilities  as  evidenced  in  these  pages 
will  stimulate  investigations  of  many  of  those  substances  which 
have  hitherto  been  studied  incompletely  or  not  at  all. 

This  volume  went  to  press  January  ist,  1907,  and  the  subject 
matter  is  brought  up  to  November,  1906. 

In  conclusion,  the  author  begs  all  indulgence  for  errors  and 
omissions,  and  will  thank  any  one  for  calling  them  to  his  attention 
or  making  suggestions  such  as  would  improve  a  possible  future 
edition  of  this  "Handbook." 

A.  S. 

WASHINGTON,  D.C.,  Feb.  22,  1907. 


ABBREVIATIONS 


Abs.  — Absolute. 

Abs.  Coef .  —  Absorption  Coefficient. 

Aq.  or  aq.  — Aqueous. 

At.  — Atmosphere. 

b.  pt.  — Boiling  Point. 

cc.  — Cubic  Centimeter. 

cone.  —  Concentrated. 

d.  —  Dextro. 

dj.  — Density. 

f .  pt.  —  Freezing  Point. 

G.,  g.,  or  gm.  —  Gram. 

Gms.  or  gms.  —  Grams. 

G.M.  or  Gm.  Mol.  —Gram  Molecule. 

/.  — Laevo. 

m.  — Meta. 

Mg.  or  mg.  —  Milligram. 

Mgs.  or  mgs.  —  Milligrams. 

Mg.  Mol.  —  Milligram  Molecule. 

Millimols.  —  Milligram  Molecules. 

Mol.  —  Molecule. 

m.  pt.  —  Melting  Point. 

N.  or  n.  —  Normal. 

o.  —  Ortho. 

ord.  —  Ordinary. 

p.  —  Para. 

ppt. —  Precipitate. 

pptd.  —  Precipitated. 

pt.  — Part. 

sat.  —  Saturated. 

sol.  —  Solution. 

Sp.  Gr.  —  Specific  Gravity. 

t°.  —  Temperature  in  degrees  C. 

temp.  —  Temperature. 

vol.  —  Volume. 

wt.  — Weight. 


vii 


ABBREVIATIONS  OF  TITLES  OF  JOURNALS 

Am.  Ch.  J.     The  American  Chemical  Journal,  Baltimore. 

Am.  J.  Sci.     American  Journal  of  Science  and  Arts,  New  Haven. 

Analyst.     The  Analyst,  London. 

Ann.     See  Liebig's  Ann. 

Ann.  chim.  anal.  appl.     Annales  de  chimie  analytique  applique"e,  Paris. 

Ann.  chim.  phys.     Annales  de  chimie  et  de  physique,  Paris. 

Ann.  Physik.     Annalen  der  Physik  und  Chemie,  Leipzig.       See  also  Pogg. 

Ann.  and  Wied.  Ann. 
Apoth.-Ztg.     Apotheker  Zeitung,  Berlin. 
Arch.  Pharm.     Archiv  der  Pharmacie,  Halle. 
Ber.      Berichte  der  deutschen  chemischen  Gesellschaft,  Berlin. 
Biedermann's    Centr.        Biedermann's    Centralblatt    fiir   Agrikulturchemie, 

u.  s.  w.,  Leipzig. 

Bull.  soc.  chim.     Bulletin  de  la  societe  chimique  de  Paris. 
Chem.  Centralbl.     Chemisches  Centralblatt,  Berlin. 
Chem.  Ind.     Die  Chemische  Industrie,  Berlin. 
Chem.  News.     The  Chemical  News,  London. 
Chem.-Ztg.     Chemiker  Zeitung,  Cothen. 
Compt.  rend.     Comptes  rendus  hebdomadaires  des  Seances  de  FAcademie 

des  Sciences,  Paris. 

Dingier  pol.  J.     Dingier' s  polytechnisches  Journal,  Stuttgart. 
Gazz.  chim.  ital.      Gazzeta  chimica  italiana,  Palermo. 

ahresber.  Chem.     Jahresbericht  iiber  die  Fortschritte  der  Chemie,  Giessen. 
.  Am.  Chem.  Soc.     Journal  of  the  American  Chemical  Society,  Easton. 
.  Anal.  Chem.     The  Journal  of  Analytical  and  Applied  Chemistry,  Easton. 
.  Chem.  Soc.     Journal  of  the  Chemical  Society  of  London. 
.  pharm.  chim.     Journal  de  pharmacie  et  de  chimie,  Paris. 
.  Physic.  Chem.     Journal  of  Physical  Chemistry,  Cornell. 
.  pr.  Chem.     Journal  fiir  praktische  chemie,  Leipzig. 
.  russ.  phys.  chem.  Ges.      Journal  of  the   Russian   Chemical   Society,    St. 

Petersburg. 

J.  Soc.  Chem.  Ind.     Journal  of  the  Society  of  Chemical  Industry,  London. 
Landw.  Vers-Stat.     Landwirthschaftlichen  Versuchs-Stationen,  Berlin. 
Liebig's  Annalen.     Justus  Liebig's  Annalen  der  Chemie,  Leipzig. 
Monatsh.  Ch.     Monatshefte  fiir  Chemie,  u.  s.  w.,  Vienna. 
Mon.  Sci.     Le  Moniteur  Scientifique,  Paris. 
Mulder.     Scheikundige  Verhandelingen  en  Onderzoekingen,   Vol.   3,   Pt.   3. 

Bijdragen  tot  de  Geschiedenis  van  Het  Scheikungig  Gebonden  Water  by 

G.  J.  Mulder,  Rotterdam,  1864. 

Pharm.  J.     Pharmaceutical  Journal  and  Transactions,  London. 
Phil.  Mag.     The  Philosophical  Magazine,  London. 
Physic.  Rev.     Physical  Review,  Cornell. 
Pogg.  Ann.     Annalen  der  Physik  und  Chemie,  edited  by  Poggendorf.     SP 

also  Ann.  Physik  and  Wied.  Ann. 
Proc.   Am.   Acad.       Proceedings  of    the   American  Academy  of  Art 

Sciences,  Boston. 

Proc.  Roy.  Soc.     Proceedings  of  the  Royal  Society  of  London. 
Rec.  trav.  chim.    Recueil  des  travaux  chimiques  des  Pays-Bas,  Leid 
Sitzber.  Akad.  Wiss.  Berlin.     Sitzungsberichte  der  koniglichen  pn 

Akademie  der  Wissenschaften  zu  Berlin. 
Sitzber.  Akad.  Wiss.  Wien.    Sitzungsberichte  der  mathematische  na 

schaftlichen   classe   der  kaiserlichen  Akademie    der  Wissensc 

Wien. 
U.  S.  P.     Pharmacopoeia  of  the  United  States,  8th  Revision,  1900 

ix 


ABBREVIATIONS    OF   TITLES    OF   JOURNALS 

Wied.  Ann.     Annalen  der  Physik  und  Chemie,  edited  by  Wiederman.     See 

also  Pogg.  Ann.  and  Ann.  Physik. 
Wiss.  Abh.  p.  t.  Reichanstalt.     Wissenschaftlichen  Abhandlung  der  physik- 

alische  technische  Reichstalt,  Charlottenburg. 
Z.  anal.  Chem.     Zeitschrift  fiir  analytische  Chemie,  Wiesbaden. 
Z.  angew.  Chem.     Zeitschrift  fiir  angewandte  Chemie,  Berlin. 
Z.  anorg.  Chem.    Zeitschrift  fiir  anorganische  Chemie,  Hamburg  and  Leipzig. 
Z.  Elektrochem.     Zeitschrift  fiir  Elektrochemie,  Halle. 

Z.  Krystallogr.     Zeitschrift  fiir  Krystallographie  und  Mineralogie,  Leipzig. 
Z.  physik.  Chem.     Zeitschrift  fiir  physikalische  Chemie,  Leipzig. 
Z.  Ver.  Zuckerind.     Zeitschrift  fiir  Rubenzucker-Industrie,  Berlin. 

The  above  abbreviations  with  a  few  necessary  exceptions  are  taken  from 
the  list  adopted  by  the  editor  of  the  Journal  of  the  American  Chemical  Society 
for  the  new  abstract  journal,  "Chemical  Abstracts,"  and  will  in  general  be 
familiar  to  many  of  those  who  use  this  volume.  In  a  large  number  of  in- 
stances Chem.  has  been  contracted  to  Ch.,  but  with  this  exception,  and  possibly  a 
few  inaccuracies  which  have  slipped  in,  the  abbreviations  of  journal  titles  used 
in  this  book  conform  to  the  above  list. 


AOENAPHTHENE     C12H10. 

SOLUBILITY  IN  SEVERAL  ORGANIC  SOLVENTS. 

(Speyers  —  Am.  J.  Sci.  [4]  14,  294,  1902.) 

NOTE.  —  In  the  original  paper  the  results  are  given  in  terms  of  gram 
molecules  of  acenaphthene,  acetamide,  acetaniiide,  etc.,  per  100  gram 
molecules  of  solvent,  at  temperatures  which  varied  with  each  solvent  and 
with  each  weighing  of  the  solutions.  The  tabulated  results  here  given 
were  obtained  by  recalculating  and  reading  the  figures  from  curves  plotted 
on  cross  section  paper. 


In  Methyl  Alcohol. 


In  Ethyl  Alcohol. 


In  Propyl  Alcohol. 


t  •. 

0 

(o)* 
81-33 

(6)*             (c)* 
1.  80      0.39 

(a) 

81.1 

(V 
1.9 

(c)   ' 

o-57 

(a) 
82.3 

(*) 
2.26 

0.88 

10 

80.40 

I 

.70      0.38 

80.3 

2 

.8 

0.84 

8l.8 

2.40 

i  .00 

20 

79.60 

2 

.25     o 

.48 

79.6 

4 

.0 

i  .20 

81.4 

3-40 

i  .35 

30 

79-00 

3 

.50     o 

.72 

79.1 

5 

.6 

1.70 

80.9 

4-75 

i  .90 

40 

78.45 

6 

.00       I 

.20 

78.7 

8 

•4 

2  .60 

80.6 

7.10 

2  .90 

50 

78.15 

9 

.00     I 

•77 

78.8 

I3 

.2 

3-90 

80.7 

ii  .10 

4.40 

60 

78.30 

ii 

.70       2 

•35 

79-4 

23 

.2 

7-00 

8l.5 

19.60 

8.20 

70 

78.60 

14.30       2 

.90 

80.75 

40 

•5 

12.50 

83-9 

37.00 

16.20 

In  Chloroform. 

In  Toluene. 

t  °. 

(«) 

(&) 

(cY 

(a) 

W 

(c) 

0 

143-8 

16. 

4     12.7 

90.7 

I3.I8 

7-9 

10 

I40.I 

20. 

6     16.0 

90.8 

18.0 

10.7 

2O 

I36-3 

27. 

o     19.5 

91  .0 

24-5 

i4-5 

30 

132.4 

34- 

o     25  .0 

91.8 

33-5 

20.5 

40 

128.0 

42. 

5     32-o 

92.7 

47.0 

28.0 

50 

123.4 

51- 

5     40-0 

94-0 

60.5 

35-7 

60 

II9-3 

62. 

5     5o-o 

95-5 

74-0 

43-5 

70 

97.2 

89.0 

52-5 

ACETAMIDE     CH3CO.NH2. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Speyers.) 


In  Water. 


t°. 

(fl) 

(6) 

(c) 

o 

105-5 

70.8 

29.6 

10 

104.9 

81.0 

34-o 

20 

104.3 

97-5 

40.8 

30 

103.7 

114.0 

47-7 

40 

103.0 

i33-o 

55-5 

50 

102.3 

154.0 

64.0 

60 

101  .6 

177-5 

74.0 

In  Ethyl  Alcohol. 


(a) 

(ft) 

(c) 

85.62 

17-3 

18.5 

86.2 

24.0 

26.0 

87-3 

31  .5 

33-8 

88.8 

40-5 

43-o 

90-7 

50.0 

53-5 

93-o 

61  .0 

64-5 

95-5 

72.0 

76.5 

ACETANILIDE     C6H5NH.COCH3. 

100  grams  H2O  dissolve  0.55  gram  at  25°,  and  5.55  grams  at  b.  pt. 


*  (a)  Weight  of  100  cc.  solution  in  grams.     *  (b)   Grams  dissolved  substance  per  100  grains  solvent. 

*  (c)  Gram  molecules  of  dissolved  substance  pe:  ioc-  gram  molecules  of  solvent. 


AOETANILIDE  a 

SOLUBILITY  OF  ACETANILIDE  IN  ORGANIC  SOLVENTS. 


In  Methyl  Alcohol. 

(Speyers.) 
In  Ethyl  Alcohol. 

In  Chloroform. 

t°. 

(a) 

(6) 

(c) 

'<«) 

<*) 

(c)  ' 

(a) 

0) 

(c)  ' 

O 

86.0 

22-7 

5-4 

84.2 

14.7 

5-o 

J50 

•3 

3 

.66 

3-24 

10 

86.4 

30.0 

7.0 

84.4 

20.  o 

6.6 

147 

•5 

7 

.80 

7.00 

20 

87-5 

41  -O 

9.8 

85-0 

27.0 

9.0 

144 

.0 

12 

.00 

10.50 

30 

89.2 

54-o 

13.2 

86.0 

36.0 

12.2 

139 

.8 

17 

.0 

15.0 

40 

gz.z 

75-5 

18.0 

87.4 

49.0 

16.2 

J35 

•4 

23 

.0 

20-  4 

50 

93-2 

107.0 

25.2 

89-5 

65.0 

22  .O 

131 

•4 

31 

.0 

27.6 

60 

95-7 

145.0 

34-o 

92.0 

87.0 

30.0 

127 

.2 

41 

.0 

36.0 

SOLUBILITY  IN  MIXTURES  OF  ETHYL  ALCOHOL  AND  WATER  AT  25°. 

(Holleman  and  Antusch  —  Rec.  trav.  chim  13,  293,  1894.) 


Vol.  %      Cms.  C8H9NO  per     on  pr 
Alcohol,     ioo  Cms.  Solvent.      SP'  Gr" 

Vol.  %      Gms.  C8H9NO  per 
Alcohol,    ioo  Gms.  Solvent. 

Sp.  Gr. 

IOO 

32 

•93 

0.8512 

55 

13 

•13 

O 

•9335 

95 

0.8737 

5o 

9 

•74 

0 

•9396 

93 

38 

.04 

0.8813 

45 

7 

•25 

0 

•9449 

90 

38 

.20 

0.8896 

40 

5 

.10 

0 

.9508 

87 

37 

.80 

0.8959 

35 

3 

•58 

0 

•9567 

85 

36 

-83 

0.8996 

31 

2 

•56 

0 

.9617 

80 

33 

.62 

0.9072 

25 

I 

•73 

o 

.9683 

75 

29 

•25 

0.9133 

20 

I 

•3o 

o 

•9736 

7o 

24 

•73 

0.9185 

15 

I 

•03 

0 

•9795 

65 

20 

.42 

0.9185 

10 

O 

•94 

0 

-9845 

60 

16 

•5i 

0.9287 

O 

0 

•54 

0 

•9970 

ACETIC  ACID 

CH3COOH. 

SOLUBILITY  IN  WATER. 

(Dahms  —  Ann.  Phys. 

[4]  60, 

122,    '97.) 

t°. 

Gms.  CHgCOOH  per 
ioo  Gms.  Solution. 

Solid 
Phase. 

t°. 

Gms.  CH3COOH  per 
ioo  Gms.  Solution. 

Solid 
Phase. 

-  5 

15  .1 

Ice 

—  20 

66.3 

CH3COOH 

—  IO 

28.2 

a 

—  io 

76- 

7 

" 

—  15 

39-5 

u 

—  o 

87.0 

« 

—  2O 

49-5 

(t 

+  10 

90. 

8 

" 

-25 

57-o 

a 

16. 

5     100.0  tr.  pt. 

tt 

-26 

.6       c8.o 

Ice- 

h  CH,COOH 

DISTRIBUTION  OF  ACETIC  ACID  BETWEEN: 
Water  and  Amyl  Alcohol  at  20°.  Water  and  Benzene  at  25°. 

(Herz  and  Fischer  —  Ber.  37,  4747,  '04)  (H.  and  F.  —  Ber.  38,  1140,  '05.) 


Gms.  CH3COOH 

G.  M.  CH3COOH 

Gms.  CH3COOH 

G.  M.  CH3COOH 

per 

IOO  CC. 

per 

IOO 

cc. 

per 

IOO  CC. 

per 

IOO  CC. 

H20 

Alcoholic 

'H20 

Alcoholic 

H20 

C6H6' 

H2O 

CeHe 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

I 

0.923 

O-OI 

0 

•0095 

5 

0.130 

0.05 

O.OOI4 

2 

1.847 

0.03 

O 

.0280 

10 

0.417 

O.IO 

0.0005 

3 

2-741 

0-05 

0 

.0460 

20 

-•55 

O-2O 

0.0030 

4 

3  694 

O.O7 

O 

.0645 

30 

3-03 

0.30 

O.O29O 

5 

4-587 

O.O9 

o 

•  0830 

40 

4-95 

0.50 

0-051 

6 

5-475 

O.II 

0 

.1010 

0.70 

0.090 

7 

6-434 

0.13 

o 

1190 

8 

7.328 

-  , 

ACETIC  AGIO 


DISTRIBUTION  OF  ACETIC  ACID  BETWEEN  WATER  AND  BENZENE. 

(Waddell  —  J.  Phys.  Ch.  2,  237,  1898.) 
Results  in  terms  of  grams  per  100  grams  solution. 


Upper  Layer. 


Lower  Layer. 


t°. 

CHaCOOH. 

C6H6. 

H20. 

25 

0.46 

99-52 

O-O2 

25 

3.10 

9^-75 

0.15 

25 

5-20 

94-55 

0.25 

25 

8.7 

90.88 

0.42 

25 

16.3 

82.91 

0-79 

25 

30-5 

67  .37 

2.13 

25 

52-5 

39.60 

7-6o 

35 

I  .2 

98.68 

0.08 

35 

5-7 

93-97 

o-33 

35 

9.0 

90.42 

0.58 

35 

45  -° 

49.00 

6.0 

35 

52.2 

39-4 

8.4 

CHaCOOH 

.    C6H6. 

H20. 

9-4 

0.18 

90.42 

28.2 

o-53 

71.27 

37-7 

0.84 

61  .46 

48-3 

1.82 

49-88 

61  .4 

6.1 

32-5 

66.0 

13-8 

20.2 

52-8 

39-6 

7.6 

16.4 

0.62 

89.98 

36.8 

1.42 

62.78 

49.0 

2.10 

48.90 

61.3 

25-5 

13.2 

52.2 

39-4 

8.4 

DISTRIBUTION  OF  ACETIC  ACID  BETWEEN  WATER  AND  CHLOROFORM: 
At  Room  Temperature.  At  25°. 

(Wright,  Thomson  and  Leon  —  Proc.  Roy.  (Herz  and  Lewy,  Rothmund  and  Wilsmore.) 

800.49,185,1891.) 


Results  in  parts  per  100  parts  of  solution. 
Upper  Layer.                             Lower  Layer. 

Cms.  CHaCOOH 
per  100  cc. 

G.  M.  CHaCOOH 
per  100  cc. 

CHaCOOH.  CHC13. 

H2O.    CHaCOOH 

.  CHC18. 

H20. 

H20 

Layer. 

CHCU 
Layer. 

H20 

Layer. 

CHCI; 

Layer. 

O 

0.84 

99- 

16 

o 

99.01 

0.99 

2 

0. 

089 

0.05 

0.0032 

6.46 

0.92 

92. 

62 

1.04 

98.24 

0.72 

4 

0. 

3J3 

0.075 

0.0062 

17.69 

0.79 

8l. 

52 

3-83 

94.98 

1.19 

6 

0. 

596 

0.100 

0.0100 

25.10 

I.  21 

73- 

69 

6.77 

91.85 

1.38 

8 

o. 

974 

0.150 

0.0198 

33-71 

2-97 

63. 

32 

1  1  .  05 

87.82 

I-I3 

10 

I. 

43° 

0-175 

0.026O 

44.12 

7-30 

48. 

58 

17.72 

80.00 

2.28 

12 

I. 

982 

0.200 

0.0325 

50.18 

15.11 

34- 

71 

25-75 

70.13 

4.12 

20 

5- 

10 

0.30 

0.070 

30 

10. 

2 

0.50 

0.170 

40 

15- 

3 

O.7O 

0.275 

50 

21. 

9 

0.80 

0-335 

52-3 

39- 

54 

0.87 

0.659 

The  figures  in  the  table  for  25°  were  read  from  the  curve  plotted 
from  the  results  of  H.  and  L.,  Z.  electro.  Ch.  u,  818,  1905,  and  of  R. 
and  W.,  Z.  phys.  Ch.  40,  623,  1902. 

The  influence  of  electrolytes  upon  the  distribution  of  acetic  acid 
between  the  aqueous  and  chloroform  layers  was  investigated  by 
Rothmund  and  Wilsmore,  and  the  following  results  expressed  in  gram 
molecules  per  liter  at  25°  were  obtained: 

Cone,  of    Cone,  of  CHaCOOH     Cone* 


ectro- 
lyte. 

Cl 
NO, 

Electrolyte 
Aq. 
Layer. 
0.463 
0.463 
0.926 
0.926 
0.316 
0.316 
0-633 
0.633 

in 

CHaCOOH    Electro-  Electrolyte 

in 

C 

HaCOOI 

H20 
Layer. 
I.I68 
1.787 

I.I68 

2.053 
I.OOO 

1-737 

Aq. 
Layer. 
0.876 
I-538 
0.8!3 
1.586 
0.936 
1.694 
0.965 
1.631 

CHCla    '      H2O 
Layer.         Layer. 
0.0907      0.946 
0.2435      1.  680 
0.0938      0.966 
0.2902      1.858 
0.0927      0.958 
0.2537      1.720 
0.0981      0.988 
0.2486      1.702 
*  Calculated 

lyte-           Aq. 
Layer. 

i  H2SO4  0.514 

1.029 

NH4N08  i.o 

I.O 

LiNO3       i.o 

I.O 
from  table  above. 

Aq. 
Layer. 
1.099 

1-555 

1.136 
1.991 

0.892 

1.513 

CHCla 
Layer. 

O.I3I5 
0.2714 

O.I3I3 
0.3481 
0.1005 
0.2581 

ACETIC  ACID  4 

DISTRIBUTION  OF  ACETIC  ACID  AT  25°  BETWEEN: 

Water  and  Carbon  Bisulphide.  Water  and  Carbon  Tetrachloride. 

(Herz  and  Lewy.)  (Herz  and  Lewy.) 

Gms.  CHaCOOH        G.  M.  CH3COOH  Cms.  CH3COOH        G.  M.  CH3COOH 

per  ipo  cc.                       per  100  cc.  per  100  cc.                   per  ipo  cc. 

'H20            CST           'H20            CS2  H20            CC14            H2O          CClT 

Layer.        Layer.          Layer.        Layer.  Layer.        Layer,        Layer.        Layer. 

65   2.64   i.i   0.45  3°    *•&   °-5   °-°3 

70   3.0    1.2   0.55  40    3-0   o-7   0-055 

75   3.3    i-2   0.80  50    4.8   0.9   0.095 

80   5.4    i-35  0.97  60    5.8    i.i   0.155 

85    6.4    1.4   i-3  7o    12.0    1.2   0.235 

76.2  25.2    1.27  0.420 

DISTRIBUTION  OF  ACETIC  ACID  AT  25°  BETWEEN: 

Water  and  Bromoform.  Water  and  Toluene. 

(H.  and  L.  —  Z.  electro.  Ch.  n,  818,  '05.)  (H.  and  F.  —  Ber.  38,  1140,  '05.) 

Gms.  CHaCOOH        G.  M.  CHaCOOH  Gms.  CH3COOH         G.  M.  CH3COOH 

per  IPO  cc.                      per  100  cc.  per  ipo  cc.                        per  100  cc. 

1^0      '  CHBr3'            '  H2O          CHBr3  'H2O     C6H5CH3          '  H2O       C6H6CH3 

Layer.       Layer.             Layer.        Layer.  Layer.    Layer.            Layer.        Layer. 

20    1.5   0.4   0-035  5  0.119   o.i  0.0025 

30    3.0    0.6   0.070  10  0.328    0.2  0.0075 

40    4.8    0.8   0.120  20  1.132    0.4  0.0260 

50    7.8    i.o   0.20  30  2.265    °-6  0.0530 

60    12.0    i.i   0.28  40  3.725    0.8  0-090 

65    15.6    1.15  0.395  50  5.841    i.o  0.140 

70      27.0        ...  60    8.344       

DISTRIBUTION  OF  ACETIC  ACID  AT  25°  BETWEEN: 

Water  and  o  or  p  Xylene.  Water  and  m  Xylene. 

(Herz  and  Fischer.)  (Herz  and  Fischer.) 


Gms.  CH3COOH 

G.  M.  CH3COOH 

Gms.  CHaCOOH 

G.M. 

CHgCOOH 

per 

100  CC. 

per 

100  CC. 

per 

100  CC. 

per  100  cc. 

H20 
Layer. 

o  or  p 
Xylene 
Layer. 

H2O 
Layer. 

o  or  p 
Xylene 
Layer. 

H20 
Layer. 

Xylene 
Layer. 

H20 
Layer. 

m 
Xylene 
Layer. 

5 

O.24 

O.I 

O.OO4 

5 

O-O6 

O.I 

0.0015 

10 

0.48 

O.2 

O-OIO 

10 

0.30 

0-2 

0.007 

20 

I-I3 

0-4 

0.025 

20 

o-95 

0-4 

0.022 

30 

2.15 

0.6 

0.047 

30 

1.91 

0.6 

O.O42 

40 

3-40 

0.8 

0.079 

40 

3-04 

0.8 

0.072 

50 

5.10 

I.O 

0.122 

50 

4-65 

i.o 

O.III 

60 

7.27 

I  .2 

0.230 

60 

6.65 

I  .2 

70 

12.52 

NOTE.  —  The  distribution  results  as  presented  in  the  original 
papers  to  which  references  are  given  in  the  above  tables,  are  reported 
in  millimolecules  per  10  cc.  portions  of  each  layer  in  the  several  cases. 
To  obtain  the  figures  given  in  the  above  tables,  the  original  results  be- 
fore and  after  calculating  to  gram  quantities  were  plotted  on  cross- 
section  paper,  and  from  the  curves  thus  obtained,  readings  for  regular 
intervals  of  concentration  of  acetic  acid  in  the  aqueous  layer  were 
selected. 


Chlor  ACETIC  ACID 


Chlor  ACETIC   ACID     CH2C1COOH. 

DISTRIBUTION  OF  CHLORACETIC  ACID  BETWEEN: 


(Herz  and  Fischer.) 


Water  and  Benzene  at  25' 


Water  and  Toluene  at  25°. 


Gms.  CH2C1COOH 

G.  M.  CH2C1COOH 

Gms.  CH2C1COOH 

G.  M.  CH2C1COOH 

per  ioo  cc. 

per  ioo  cc. 

per  ioo  cc. 

per  ioo  cc. 

H2O            C6H6 

H2O             C(jHe 

Jtl2vJ          CensLrls 

H2O         C6H5CH3 

Layer.         Layer. 

Layer.          Layer. 

Layer.        Layer. 

Layer.          Layer. 

0.25*      8.69 

0.0025      0-090 

o.i*      5.22 

o.ooi     0.055 

o-5       15-59 

0.005         0.155 

0-5         20.31 

O.005       O-2O 

i.o       27.87 

o.oio      0-28 

i.o       34.87 

o.oio     0.36 

1.5       41.10 

0-015       0.415 

1-5         49.14 

O.OI5       0.50 

2.0         52.90 

O-O2            O-54 

2  .  0         60  •  46 

O-O2         O.62 

3.0       68.01 

0.03            0.70 

3-0          72.28 

0-03         0-77 

4-o       76.52 

O.O4            O-79 

4-0         81.72 

0-04         0-85 

5-O         86.94 

0-05         0.90 

DISTRIBUTION  OF  CHLORACETIC  ACID  BETWEEN: 

(Herz  and  Lewy.) 


Water  and  Chloroform  at  25* 


Water  and  Bromoform  at  25°. 


Gms.  CH2C1COOH 

G.  M.  CH2C1COOH 

Gms.  CH2C1COOH 

G.  M.  CH2C1COOH 

per 

IOO   CC 

per  ioo  cc. 

per  ioo  cc. 

per  ioo  cc. 

H20 

CHC13 

H2O 

CHClg    ' 

H20 

CHBr3 

H20 

CHBrs 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

5* 

0.283 

0-05 

O.OO25 

40* 

0.850 

o-45 

O.OII 

10 

0.614 

0.10 

o  •  0060 

50 

1.889 

0.50 

0-0165 

20 

1.  088 

O.2O 

0.0135 

60 

2.994 

0.60 

O.O28 

40 

2.948 

0-40 

O.O29 

70 

4.241 

0.70 

0.040 

50 

3.684 

O-6o 

0.045 

80 

5.620 

0.80 

0-053 

60 

4.440 

0.70 

0.061 

90 

7.560 

0.90 

0-067 

70 

7.086 

o-75 

0.077 

91  .6 

11.340 

0.97 

O.I2O 

DISTRIBUTION  OF  CHLORACETIC  ACID  BETWEEN: 

(Herz  and  Lewy.) 


Water  and  Carbon  Bisulphide 
at   25°. 


Water  and  Carbon  Tetra- 
chloride  at  25°. 


Gms.  CHzClCOOH 
per  ioo  cc. 

G.  M.  CH2C1COOH 
per  ioo  cc. 

Gms.  CH2C1COOH 
per  ioo  cc. 

G 

.  M.  CH2C1COOH 

per  ioo  cc. 

'H2O 

CS2  ' 

H20 

Cb2 

H20 

ecu 

H20 

ecu 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

60* 

0 

.426 

0.6 

O 

.OO42 

90* 

I 

.417 

0 

•95 

0.0150 

80 

0 

.691 

0.8 

0 

.007 

95 

2 

.031 

I 

.00 

0.0195 

90 

O 

.803 

I.O 

o 

.009 

IOO 

2 

•645 

I 

•05 

O.O27O 

IOO 

I 

.040 

1.05 

o 

•0105 

105 

4 

.26 

I 

.10 

0.0415 

105 

I 

.464 

1.  10 

o 

.015 

106.7 

5 

.19 

I 

•13 

0.0550 

106.7 

I 

.890 

1-13 

o 

,020 

See  Note,  page  4- 


Chlor  ACETIC  ACIDS 


SOLUBILITY  OF  MONOCHLOR,  DICHLOR,  AND  OF  TRICHLORACETIC  ESTER 
IN  AQUEOUS  ALCOHOL  AT  ROOM  TEMPERATURE. 

(Bancroft  —  Phys.  Rev.  3,  193,  1895-96,  from  results  of  Pfeiffer,  Z.  physik.  chena.  9,  469,  '92.) 


cc.  Ethvl 
Alcoholin 

cc.  H2O  added  to  cause  separation  of  a  second  phase 
in  mixtures  of  the  given  amis,  of  Alcohol  and  3  cc.  of  : 

Mixtures. 

CHaClCOOC2H5. 

CHC12COOC2H5 

CC13COOC2H5. 

3 

1.32 

O.QO 

0.65 

6 

4-OI 

2-45 

1.  80 

9 

7-30 

4-33 

3.02 

12 

10.78 

6.60 

4.50 

15 

i6.!6 

9.  2O 

6.50 

18 

22.16 

.  .  . 

21 

28.74 

a  AOETNAPHTHALIDE     C2H(ONH(C10H7). 

SOLUBILITY  IN  MIXTURES  OF  ALCOHOL  AND  WATER  AT  25°. 

(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  289,  1894.) 


Vol.% 
Alcohol. 

Gms.  per 
100  Gms. 
Solvent. 

Sp.  Gr.  of 

Solutions. 

Vol.% 
Alcohol. 

Gms.  per 
100  Gms. 
Solvent. 

Sp.  Gr.  of 
Solutions. 

100 

4-02 

0.7916 

65 

I.78 

0.8977 

95 

4-31 

0.8150 

60 

1-44 

0.9091 

90 

4-II 

0.8344 

55 

1.02 

0.9201 

85 

3-69 

0.8485 

5° 

0.71 

0.9290 

80 

3-18 

0.8624 

35 

0.25 

0-9537 

75 

2-73 

0-8761 

20 

O.O9 

0.9717 

70 

2.31 

0.8798 

10 

0.04 

0.9841 

ACETONE  (CH3)2CO. 

SOLUBILITY  OF  ACETONE  AT  25°  IN  AQUEOUS  SOLUTIONS  OF: 
Electrolytes.  Non-Electrolytes. 

(Bell  — J.  Phys.  Ch.  9,  544,  1905;  Linebarger  —  Am.  Ch.  J.  14,  380,  1892.) 


Gms.  Electro- 
lyte per 

Gms.  (CH3)2CO  per  100  Gms. 
Solvent  in  Solutions  of: 

Gms.  Non-    Gms.  (CH3)2CO  per  100  Gms. 
Electrolyte           Solvent  in  Solutions  of: 

Solution. 

K2C03 

Na2CO3  (NH4)2CO3  MgCO3       Aq.  Solution.   doH8* 

Anethol.*  (C6H5)2CO. 

I 

•25 

. 

.  .  . 

83- 

5 

5 

92.5 

103.0 

90.0 

2 

•50 

. 

51.0 

IIO.O 

65- 

0 

10 

117.0 

123.0 

108.5 

5 

•  CO 

65 

.0 

38.0 

73-5 

47- 

o 

20 

137.0 

144-5 

126.0 

7 

•5 

46 

•5 

27-5 

57-o 

38. 

O 

30 

148.5 

155-0 

i33-o 

10 

•  0 

34 

•5 

19-5 

44-5 

29. 

0 

40 

J55-5 

162  -O 

136.0 

12 

•5 

25 

•5 

14.0 

35-o 

50 

159-5 

166.0 

135-5 

15 

.0 

18 

.0 

9-0 

28.0 

.  . 

. 

60 

160.2 

165.0 

I3I-5 

20 

.0 

8 

.0 

2-7 

. 

70 

i55-o 

158.0 

123.0 

25 

.0 

3 

•7 

. 

80 

108.5 

30 

•  O 

i 

.6 

. 

90 

82.0 

*  Anethol  =  p  Propenylanisol  CHs.CHiCHUK^OCHs.    Naphthalene  results  at  35°. 

NOTE.  —  The  original  results  were  recalculated  and  plotted  on  cross- 
section  paper.  From  the  curves  so  obtained  the  above  table  was 
constructed.  See  also  Note,  page  7. 


ACETONE 


SOLUBILITY  OP  ACETONE  IN  AQUEOUS  SOLUTIONS  OF  CARBOHYDRATES. 

(Krug  and  McElroy  —  J.  Anal.    Ch.  6,  184,  '92;  Bell  —  J.  Phys.  Ch.  9,  547,  '05.) 


Per  cent 
Sugar. 

IO 
20 
30 

35 
40 

45 
5o 
55 
60 

65 
70 


In  Aqueous  Solutions  of  Cane  Sugar. 

Gms.  (CH3)2CO  per  100  Gms.  Sugar  Solution  at: 


15°. 

20°.                      25°.                 30°. 

35°. 

—  \ 
40°. 

597-2 

581.8 

574-8 

272.5 

250.0 

251.8 

172.4 

150.0 

150.6 

96.4 

92.8 

89.8 

71.9 

68.8 

65-7 

50.8 

48.1 

45-9 

35-8 

33-8 

32-5 

25.2 

24.2 

23-4 

18.3 

17.7 

17.0 

13.2 

12.8 

12-5 

no 

85 

62 
42 
29 


In  Aqueous  Dextrose  Solutions. 


In  Aqueous  Maltose  Solutions. 


Per 

cent 

Gms 

,  (CH3)2CO 

Solvent 

per 
at: 

ioo  Gms. 

Per 

cent 

Gms.  (CH3)2CO  per  ioo  Gms. 
Solvent  at: 

Dextrose. 

15°. 

25°- 

3S°- 

Maltose. 

i5°-                 25°. 

35°-' 

10 

736 

•7 

747 

9 

76l 

•5 

IO 

353-6 

348. 

,i 

342.0 

2O 

255 

•3 

247 

•7 

240 

.8 

20 

185.4 

181, 

,2 

176.9 

30 

157 

•5 

149 

.8 

142 

•5 

30 

119.9 

116 

.0 

112  .4 

40 

86 

•9 

79 

.6 

74' 

40 

78.4 

74 

•7 

70-5 

50 

36 

.2 

33 

.0 

31 

.2 

50 

46.2 

42 

9 

39-8 

NOTE.  —  The  above  determinations  were  made  by  adding  successive 
small  quantities  of  acetone  to  mixtures  of  known  amounts  of  water 
and  the  carbohydrate,  and  noting  the  point  at  which  a  clouding  due 
to  the  separation  of  a  second  phase  occurred.  This  method  was  also 
used  for  the  solubility  of  acetone  in  the  aqueous  electrolyte  solutions 
(see  previous  page).  In  the  case  of  the  aqueous  non-electrolyte 
solutions,  however,  successive  small  amounts  of  water  were  added  to 
mixtures  of  known  amounts  of  acetone  and  the  non-electrolyte. 


DISTRIBUTION  OF  ACETONE  BETWEEN  WATER  AND  BENZENE  AT  25°. 

(Herz  and  Fischer  —  Ber.  38,  1142,  '05.) 

Gms.  (CH3)2CO  per  ioo  cc.  G.  M.  (CH3)2CO  per  ioo  cc. 

C6H6  * 
Layer. 

0.025 
0-047 

o-975 
0.150 
0.215 
0.275 


Aq. 
Layer. 

C6H6 
Layer. 

Aq. 
Layer. 

I* 

I  .20 

O.O25* 

5 

4.17 

O.O5 

10 

10.15 

O.IO 

IS 

15  .59 

0.15 

20 

22.50 

O-2O 

0.25 

* 

See  Note,  page  4. 

ACET-PHENETIDINE  8 

ACET-PHENETIDINE  p  (PHENACETINE  s 

SOLUBILITY  IN  WATER,  ALCOHOL,  ETC. 

(U.  S.  P.) 
Gms.  C8H4(OC2HS)NHCH3CO  per  100  Gms. 


25 
b.pt. 


H20. 
0.108 
1-43 


C2H5OH. 

8-33 

5O.O 


(CH3)20. 


CHC1,. 


ACET-TOLUIDE  p  CH3.C6H4NH.C2H3O. 

SOLUBILITY  IN  MIXTURES  OF  ALCOHOL  AND  WATER  AT  25' 

(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  288,  '94.) 


Alcohol. 

Gms.  per 
loo  Gms. 
Solvent. 

Sp.  Gr. 
of 
Solutions. 

IOO 

IO.I8 

o  .  8074 

95 

10-79 

0.8276 

90 

IO.62 

0.8440 

85 

9.62 

0.8576 

80 

8-43 

0.8685 

75 

7.04 

0.8803 

70 

5.81 

o  .  8904 

65 

4-39 

0.9021 

60 

3-59 

0.9II5 

55 

2  .69 

0.9207 

Vol.  % 
Alcohol. 

Gms.  per 
TOO  Gms. 
Solvent. 

Sp.  Gr, 

of 
Solutions. 

50 

1.92 

0.9306 

45 

I.4I 

0.9380 

40 

0.96 

0.9460 

35 

0.66 

0.9544 

25 

0.31 

0.9668 

20 

0.23 

0-9725 

15 

0.16 

0.9780 

5 

0.13 

0.9903 

o 

O-I2 

0.9979 

ACETYLENE  C2H2. 


SOLUBILITY  IN  WATER. 


(Winkler  ;  see  Landolt  and  Bornstein's  Tabellen,  3d  ed.  p.  604,  '05.) 


O 

5 
10 

15 

20 

25 
30 


1.49 


1.03 

o-93 
0.84 


O.20 
0.17 
0.15 
0.13 
O-I2 
O.II 
0.09 


a,  "  Absorption  Coefficient,"  =  the  volume  of  gas  (reduced  to  o° 
and  760  mm.  pressure)  taken  up  by  one  volume  of  the  liquid  at  the 
given  temperature  when  the  partial  pressure  of  the  gas  equals  760  mm. 
mercury. 

<7,  "  Solubility,"  =  the  amount  of  gas  in  grams  which  is  taken  up  by 
loo  grams  of  the  pure  solvent  at  the  given  temperature  if  the  total 
pressure,  i.e.,  the  partial  pressure  of  the  gas  plus  the  vapor  pressure  of 
the  liquid  at  the  absorption  temperature  is  760  mm. 


9  ACETYLACETONE 

ACETYLACETONE  CH3COCH2COCH,. 

SOLUBILITY  IN  WATER. 

(Rothmund  —  Z.  phys.  Ch.  26,  475,  '98.) 

Cms.  CH8COCH,COCH8  per  100  Cms. 


30 
40 

50 
60 
70 
80 

87.7  (crit.  temp.)  56.8 

NOTE.  —  Weighed  amounts  of  water  and  acetylacetone  were  placed  in 
small  glass  tubes,  which  were  then  sealed  and  slowly  heated  until  the 
contained  mixtures  became  homogeneous.  The  temperature  was  then 
allowed  to  fall  very  gradually  and  the  point  noted  at  which  cloudiness 
appeared.  This  point  was  accurately  established  for  each  tube  by  repeated 
trials.  The  curve  plotted  from  these  determinations  shows  two  percentage 
amounts  of  acetylacetone  which  cause  cloudiness  at  each  temperature 
below  the  critical  point.  Of  these  two  points,  for  each  temperature,  one 
represents  the  aqueous  layer,  i.e.,  the  solubility  of  acetylacetone  in  water; 
and  the  other  represents  the  acetylacetone  layer,  i.e.,  the  solubility  of 
water  in  acetylacetone.  This  method  is  known  as  the  "  Synthetic  Method," 
and  yields  results  in  harmony  with  those  obtained  by  the  analytical  method, 
i.e.,  by  analyzing  each  layer  after  complete  separation  occurs. 


H20 
Layer. 

Acetyl  Acetone 
Layer. 

15.46 
I7-58 

95-02 
93.68 

2O.22 
23-23 

91.90 
89.41 

27.10 
33-92 

78.82 

AOONITINE  (Amorphous)  C34H47NOn. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(At  25°  U.S.P.;  at  i8°-22°,  Miiller  —  Apoth.-Ztg.  18,  2,  '03.) 


Gms.  C34H4jNOi  per  .         Cms.  CsJL^NOn  per 

Solvent.  IOQ  Gms.  Solvent  at:  Solvent.  100  Gms.  Solvent  at: 

i8°-22°.  25°.  i8°-22°.     '         IpT 

Water  .    .    .  0.054        0.031  Benzene       .......  J7-85 

Alcohol    .....  4.54  Carbon  Tetrachloride   1.99 

Ether   ...  1.44          2.27  Petroleum  Ether  .    .     0.023      0.028 


ADIPIO  ACID  (Normal)   (CH2)4(COOH)2. 

100  grams  H2O  dissolve  1.44  grams  adipic  acid  at  15°. 

(Henry  —  Compt.  rend.  99,  1157,  '84;  Lamouroux  —  Ibid.  128,  998,  '90-) 


AIR. 


10 


AIR 


SOLUBILITY  IN  WATER. 

(Wiakler  —  Her.  34,  1409,  '01;  see  also  Peterson  and  Sondern  —  Ber.  22,  1439,  '89.) 

cc.*  of  atmospheric  O  and  N  per  liter  of: 
Dist.  H2O  (at  760  mm.).        Sea  Water  (at  760  mm.). 


t". 

a. 

&  . 

Oxygen. 

Nitrogen. 

Oxygen. 

Nitrogen. 

0 

0.02881 

0.02864 

10.19 

18.45 

7-77 

14.85 

5 

•02543 

.02521 

8.91 

16.30 

6-93 

J3-32 

10 

.02264 

.02237 

7.87 

14.50 

6.29 

12  .06 

J5 

.02045 

.O2OII 

7-04 

13.07 

5-7o 

II  .05 

20 

.01869 

.01826 

6-35 

II  .91 

IO.25 

25 

.01724 

.01671 

5-75 

10.96 

9.62 

30 

.01606 

•01539 

5-24 

IO.I5 

40 

.01418 

•CI3IS 

4-48 

8.67 

5o 

.01297 

.01140 

3.85 

7-55 

60 

.01216 

.00978 

3-25 

6.50 

80 

.01126 

.00600 

1.97 

4-03 

00 

.01105 

.  ooooo 

o.oo 

0-00 

B  =  "  Coefficient  of  Absorption,"  i.e.,  the  amount  of  gas  dissolved 
by  the  liquid  when  the  pressure  of  the  gas  itself  without  the  tension 
of  the  liquid  amounts  to  760  mm. 

Bf  =  "  Solubility,"  i.e.,  the  amount  of  gas,  reduced  to  o°  and  760 
mm.,  which  is  absorbed  by  one  volume  of  the  liquid  when  the  barometer 
indicates  760  mm.  pressure. 

*  Reduced  to  o°  and  760  mm. 

SOLUBILITY  OF  AIR  IN  AQUEOUS  SULPHURIC  ACID  AT  18°  AND  760  MM. 

(Tower  — Z.  anorg.  Ch.  50,  382,  '06.) 

Wt.  %  H2SO4  98  90  80  70  60          50 

Solubility  Coef.       0.0173    0.0107    0.0069    0.0055    0.0059    0.0076 

SOLUBILITY  OF  AIR  IN  ALCOHOL,  ETC. 

(Robinet  — Compt.  rend.  58,  608,  '64.) 
Solvent. 

Oil  of  Lavender .    . 
Oil  of  Turpentine  . 
14.0 


Solvent. 


Vols.  Air  per  100 
Vols.  Solvent. 


Alcohol  (95 .  i%)    .    .   14.1 

Petroleum 6.8 

Benzene  . 


Vols.  Air  per  100 
Vols.  Solvent. 

.  .    6.9 

.     .    24.2 


ALANINE     («  Aminopropionic  Acid)   CH3CH(NH2)COOH. 

SOLUBILITY  IN  MIXTURES  OF  ALCOHOL  AND  WATER  AT  25°. 

(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  297,  '94.) 


Vol.% 
Alcohol. 

Gms.  per 
100  Gms. 
Solvent. 

Sp.  Gr.  of 
Solutions. 

0 

16.47 

I  .0421 

5 

14-37 

I.03II 

IO 

12.43 

I  -O2OO 

15 

10.49 

I  .0101 

20 

8.48 

0.9984 

25 

7.11 

0-9886 

31 

5-53 

0.9761 

Vol.  % 

Gms.  per 

Sp.  Gr.  of 

Alcohol. 

100  Gms. 
Solvent. 

Solutions. 

35 

4.91 

0.9670 

40 

3-89 

0-9577 

50 

2.38 

0-9355 

60 

i-57 

0.9102 

70 

0.85 

0.8836 

80 

o-37 

o  8556 

ii  ALDEHYDE 

ALDEHYDE. 

SOLUBILITY  OF  p   FORMALDEHYDE  (TRIOXYMETHYLENE)    IN  AQUEOUS 
SODIUM  SULPHITE  SOLUTIONS  AT  20°. 

(Lumiere  and  Seyewetz  —  Bull.  soc.  chim.  [3]  27,  1213,  '02.) 

Grams  Sodium  Sulphite  per  100  cc.  H2O  5         10        20        28 

Gms.  Trioxymethylene  per  100  cc.  solution       22         24        26        27 

100  gms.  H2O  dissolve  12.5  paraldehyde  at  25°,  and  6.6  gms.  at  b.  pt. 

ALCOHOLS. 

SOLUBILITY  OF  AMYL  ALCOHOL  IN  WATER  AT  22°. 

(Herz  —  Ber.  31,  2671,  '98.) 

ioo  cc.  water  dissolve  3.284  cc.  amyl  alcohol.  Sp.  Gr.  of  solu- 
tion =  0.9949,  Volume  =  102.99  cc. 

ioo  cc.  amyl  alcohol  dissolve  2.214  cc.  water.  Sp.  Gr.  of  solu- 
tion =  0.8248,  Volume  =  101.28  cc. 

Sp.  Gr.  of  H2O  at  22°  =  0.9980 ;  Sp.  Gr.  of  amyl  alcohol  at  22°=  0.8133. 

SOLUBILITY  OF  AMYL  ALCOHOL  IN  WATER  AT  DIFFERENT  TEMPERA- 
TURES, "  SYNTHETIC  METHOD"  (see  Note,  page  9). 

(Alexejew  —  Ann.  phys.  Chem.  28,  305,  '86.) 
Gms.  CsHnOH  per  ioo  Gms.  Gms.  CcHnOH  per  ioo  Gms. 

to  ' Aqueous  Alcoholic  '  to  '  Aqueous  Alcoholic" 

Layer.  Layer.  Layer.  Layer. 

08  97  ioo  2.0  80 

20                6  94  120  4.0  77 

40               4  90  140  7-o  73 

60                2  87  150  9.0  72 

80  1.5  83 

SOLUBILITY  OF  AMYL  ALCOHOL  IN  AQ.  ETHYL  ALCOHOL  SOLUTIONS. 

(Bancroft  —  Phys.  Rev.  3,  193,  '95-96.) 
~r   Fthvl  cc.H2O  added  to  cause  Separation  of  a 

4i     u  1  Second  Phase  in  Mixtures  of  the  given 

Alcohol  Amounts  of  Ethyl  Alcohol  and  3  cc. 

in  Mixture.  Portions  of  Amvl  Alcohol  at: 

9.1°.  19.2°. 

3  !3-21  3-5o 

6  !o-3S  10. 80 

9  18.34  19-10 

12  27.47  29-15 

15  4I-25  43-15 

NOTE.  —  The  effect  of  various  amounts  of  a  large  number  of  salts 
upon  the  temperature  (39.8°)  at  which  a  mixture  of  20  cc.  of  amyl 
alcohol  +  20  cc.  of  ethyl  alcohol  +  32.9  cc.  of  water  becomes  homo- 
geneous has  been  investigated  by  Pfeiffer  (Z.  phys.  Ch.  9,  444,  '92). 
The  results  are  no  doubt  of  interest  from  a  solubility  standpoint,  but 
their  recalculation  to  terms  suitable  for  presentation  in  the  present 
compilation  has  not  been  attempted. 

SOLUBILITY  OF  ISOAMYL  ALCOHOL  IN  WATER. 

0    Gms.  Iso  Amyl  Alcohol  per  ioo  Gms.  Q, 

H2O  Layer.  Alcoholic  Layer. 

13.7       2.0  ...  Balbrano  —  Ber.  9,  1437, '76 

16.5       2.5  92.9  Wittstein  —  Jahrb.  408,  '62 

22  2.61  97.36  Herz  — Ber.  31,  2669, '98 


to 

Aqueous 

Alcoholic 

. 

Layer. 

Layer. 

—  20 

27 

66 

—  10 

28 

60 

0 

27-5 

56 

10 

26.O 

57 

20 

22-5 

60 

30 

18 

63-5 

40 

16 

65-5 

60 

I3 

67 

80 

i5 

63 

100 

20 

52 

loycrit. 

temp.         33 

120 

130 

133  crit 

.  temp. 

ALCOHOLS  12 

SOLUBILITY  OF  BUTYJ^  ALCOHOLS  IN  WATER,  "  SYNTHETIC  METHOD  " 
(see  Note,  page  9). 

(Alexejew  —  Ann.  phys.  Chem.  28,  305,  '86.) 

Secondary  Butyl  Alcohol  I  so  Butyl  Alcohol 

and  Water.  and  Water. 

Cms.  Secondary  Butyl  Alcohol  per  100  Gms.         Cms.  Iso  Butyl  Alcohol  per  100  Cms. 

Aqueous  Alcoholic 

Layer.  Layer. 


13    85 

9      84 

7-5     83 
7      82 

7  77-5 

8  72 

16      62 
28      50 
40 

DISTRIBUTION  OF  ETHYL  ALCOHOL  BETWEEN  WATER  AND  BENZENE 

AT  25°. 

(Taylor  — J.  Phys.  Ch.  I,  468,  '97.) 

Composition  of  10  cc.  of  Upper  Layer.  Composition  of  10  cc.  Lower  Layer. 

CflHa.             HaCT C2H5OH.                        'CeH6.  H^O  C2H6OH. 

5.92            0.60           3.48                         4.37  1.07            4.56 

6.43            0.48           3-09                         3.54  I.4I            5.05 

7.40           0.29            2.31                         2.04  2.27            5.69 

8.13            0.17            1.70                         I. 08  3.22            8.70 

8.65        o.io         1.25  0.59        4-06        5.35 

9.05  0.06  0.89  0.28  4.99  4.73 

ALUMINIUM  CHLORIDE     A1C13  -  6  H2O. 

SOLUBILITY  IN  WATER. 

(Gerlach  — Z.  anal.  Ch.  8,  250,  '69.) 

ioo  gms.  saturated  solution  contain  41.13  gms.  A1C13  at  15°,  Sp.  Gr0 
of  solution  =  1.354. 

ALUMINIUM  SULPHATE     A12(SO4)3  •  18  H2O. 
SOLUBILITY  IN  WATER. 

(Poggiale  —  Ann.  chim.  phys.  [3]  8,  467,  '43.) 

Gttn.  A12(SO4)3  per  ioo  Gms.  Gms.  A12(SO4)3  per  ioo  Gms. 

t°.  Water.         Solution.  t°.  Water.         Solution/ 

o        31.3         23.8  60        59.1         37.2 

10        33.5         25.1  70        66.2        39.8 

20  36.1  26.7  80  73-1  42.2  y 

30  40.4  28.8  90  80.8  44.7 

40         45.7         31.4  ioo        89.1         47.1 

So         52-1         34-3 

ioo  gms.  of  a  saturated  solution  of  aluminium  sulphate  in  glycol  con- 
tain 14.4  gms.  A12(SO4)3.  (de  Coninck— Bull.  acad.  roy.  Belgique,  359,  '05.) 


ALUMS 


ALUMS. 


SOLUBILITY  OP  AMMONIUM  ALUM  AND  OP  POTASSIUM  ALUM 
IN  WATER. 

(Mulder ;    Poggiale  —  Ann.  chim.  phys.  [3]  8,  467,  '43;  Locke  —  Am.  Ch.  J  26,  174,  '01;  Marino 
Gazz.  chim.  ital.  35,  II,  351,  '05;  Berkeley  —  Trans.  Roy.  Soc.  203  A,  214,  '04.) 


Ammonium  Alum. 


Potassium  Alum. 


t°. 

Gms.  (NHJt 
A12(S04)4 

Gms.  (NH4)2 
A12(S04)424H20 

G.M.(NH4)2 
A12(S04)4 

Gms.  K2 
A12(S04)4 

Gms.  K2           G.  M.  K2 
A12(S04)424H20    A12(S04)4 

per  100  g. 

per  100  g. 

per  100  g. 

per  100  g. 

per  100  ST. 

per  100  fir. 

H20. 

H20. 

H20. 

H20. 

H2O. 

H2O. 

o 

2.10 

3-90 

O.OO44 

3-° 

5-65 

0-0058 

5 

3-50 

6.91 

O.OO74 

3-5 

6.62 

0.0068 

10 

4-99 

9-52 

O.OI05 

4-0 

7.60 

0.0077 

15 

6.25 

12.66 

0.0132 

5-° 

9-59 

0.0097 

20 

7-74 

I5-I3 

0.0163 

5-9 

ii  .40 

O.OII4 

25 

9.19 

19.19 

O.OI94 

7-23 

14.14 

O.OI4O 

30 

10.94 

22  -OI 

0.0231 

8-39 

16.58 

O.OI62 

40 

14.88 

30.92 

0-0314 

11.70 

23-83 

0.0227 

5o 

20.  IO 

44-10 

0.0424 

17.00 

36.40 

0.0329 

60 

26.70 

66.65 

0-0569 

24-75 

57-35 

0.0479 

70 

40.0 

110.5 

0.0774 

80 

71.0 

321-3 

0-1374 

90 

109.0 

2275.0 

0.2IIO 

92  5 

119.0 

00 

0-2313 

95 

109.7 

00 

0.2312 

NOTE. — The  potassium  alum  figures  in  the  preceding  table  were 
taken  from  a  curve  plotted  from  the  closely  agreeing  determinations  of 
Mulder,  Locke,  Berkeley,  and  Marino.  For  the  higher  temperatures 
(above  60°),  however,  the  results  of  Marino  are  lower  than  those  of 
the  other  investigators,  and  are  omitted  from  the  average  curve. 

Locke  called  attention  in  his  paper  to  the  fact  that  Poggiale 's  results 
upon  ammonium  and  potassium  alum  had  evidently  become  inter- 
changed through  some  mistake.  This  explanation  is  entirely  sub- 
stantiated, not  only  by  Locke's  determinations,  but  also  by  those  of 
Mulder  and  Berkeley.  The  ammonium  alum  figures  given  above  were 
therefore  read  from  Poggiale's  potassium  alum  curve,  with  which 
Locke's  determination  of  the  solubility  of  ammonium  alum  at  25°  is  in 
entire  harmony. 


SOLUBILITY  OF  AMMONIUM  ALUM  IN  PRESENCE  OF  AMMONIUM  SUL- 
PHATE AND  IN  PRESENCE  OF  ALUMINIUM  SULPHATE  IN  WATER. 


Mixture  Used. 


(Riidorff  —  Ber.  18,  1160,  '85.) 

100  Gms.  Saturated  Solution  Contain: 


Grams  (NH4)2SO4  +  Grams 

Saturated  Ammonium  Alum  at  18.5° 1.42  3.69 

20  cc.  above  sol.  +  6  gms.  cryst.  A12(SO4)3  .    .    .     0.45  16.09 

20  cc.  above  sol.  +  4  gms.  cryst.  (NH4)2SO4.    ..   20.81  0.29 


ALUMS  14 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  ALUM  AND  ALUMINIUM  SUL- 
PHATE AND  OF  POTASSIUM  ALUM  AND  POTASSIUM  SULPHATE 
IN  WATER. 


(Marino  —  Gazz.  chim.  ital.  35,  II,  351,  '05.) 


to 

Gms.  per  1000  Gms.  H2O. 

Gm.  Mols.  per  i  ooo  Mols.  H2O. 

• 

Al2(S04)3.i8H20. 

K2SO4. 

Al2(SO4)3-i8H2O. 

K2S04.' 

o 

243-73 

23-45 

6.1 

2-3 

20 

824.25 

30.85 

15.1 

3.1 

35 

911  .02 

35-29 

24.1 

3-6 

1243-21 

59-55 

33-5 

6.1 

65 

1598.00 

ii9-43 

43.1 

12.6 

77 

1872  .11 

183.80 

5o-5 

18.9 

0 

5.06 

75  -83 

O.I 

7-8 

°-5 

8.66 

75  •I8 

O.2 

7-7 

5- 

16.07 

85.78 

0-4 

8.8 

10 

18.52 

96.50 

o-5 

99 

15 

20.56 

109.30 

o-55 

II.  2 

39.60 

147-8 

I  .0 

15.2 

40 

73-88 

163.1 

1.9 

16.8 

50 

126.0 

195-4 

3-4 

20.1 

60 

249.7 

238.8 

6.7 

24.6 

7o 

529.0 

323.7 

14.2 

3^-6 

80 

1044.0 

517-27 

28.1 

S3  -4 

Solid 
Phase. 


K2A12(S04)2.24H20 

+  A12(S04)3 


K2A12(S04)2.24H20 
+  K2S04 


SOLUBILITY  OF  MIXTURES   OF  POTASSIUM  ALUM   AND  OF  THALLIUM 
ALUM  IN  WATER  AT  25°. 

(Fock  — Z.  Kryst.  Min.  28,  397,  '97.) 

K2A12(SO4)4.24H2O ;  T12A12(SO4)4.24H2O. 


Con 

iposition  of  ; 

A_  .    ._ 

solution. 

Solid  Phase 

KAl(SO4)2J>er  Liter. 

T1A1(SO4)2  per  Liter. 

Mol.%            Sp.  Gr.  of 

Mol.  %  of 
Potassium 

Grams. 

Mg.  Mols. 

Grams. 

Mg.  Mols. 

KA1(S04)2.         Solutions. 

Alum. 

69.90 

270.5 

o.oo 

o.oo 

100              1-0591 

IOO-O 

74-56 

288.2 

0.48 

I-I3 

99.61 

.0601 

99-32 

67.90 

262.8 

1.72 

4.07 

98.48 

.0598 

96.84 

65-30 

252.7 

4-52 

10.67 

95-95 

.0603 

90.84 

64-95 

251.4 

9.60 

22  .67 

9i-73 

.0605 

82.94 

53-23 

205-9 

18.44 

43-56 

82.54 

.0609 

68.24 

45-32 

175-4 

24.60 

58.10 

75-12 

.0609 

58.23 

38.02 

147.2 

32.48 

76.75 

65-73 

.0611 

46.72 

34-54 

J33-6 

35-59 

84.10 

61.36 

.0611 

44-23 

28-35 

109.7 

42.99 

101  .60 

5r-93 

.0623 

32-07 

10.94 

42.4 

66.12 

156.2 

21-34 

.0654 

7-94 

o.oo 

o.o 

75-46 

178.3 

o.oo 

.0674 

O-OO 

ALUMS 


SOLUBILITY  OP  SODIUM  ALUM  IN  WATER. 


100  gms.  H2O  dissolve  51.0  gms.  (?anhy.)  Al2Na2(SO4)4.24H2O  at  16°. 

(Auge—  Compt.  rend,  no,  1139,  '90.) 

ioo  gms.  H2O  dissolve  no.o  gms.  Al2Na2(SO4)4.24H2O  at  o°. 

(Tilden  —  J.  Ch.  Soc.  (Lond.)  45,  269,  '84.) 


SOLUBILITY  OF  CAESIUM  ALUM,  RUBIDIUM  ALUM,  AND  OF  THALLIUM 

ALUM  IN  WATER. 

(Setterburg  —  Liebig's  Annalen,  ail,   104,  '82;  Locke  —  Am.  Ch.  J.  26,  183,  '01;  Berkeley  —  Trans. 

Roy.  Soc.  203  A,  215,  '04.) 


Caesium  Alum. 
Gms.  per  ioo  Gms.  H2O. 


Rubidium  Alum. 
Gms.  per  ioo  Gms.  H2O. 


fc    . 

Al2Cs2(S04)4. 

Al2Cs2(S04)4 
.24H20. 

Al2Rb2(S04)4. 

AlaRb2(S04)4 
.24H20. 

0 

O.2I 

o-34 

0.72 

I  .21 

5 

0.25 

0.40 

0.86 

1.48 

10 

0.30 

0.49 

1.05 

1.81 

20 

O.4O 

0.65 

1.50 

2-59 

25 

0.50 

0.81 

i.  80 

3.12 

30 

O-6o 

o-97 

2.20 

3-82 

40 

0.85 

1.38 

3-25 

5-69 

50 

1.30 

2.  II 

4-8o 

8.50 

60 

2-00 

3-27 

7-40 

I3-36 

70 

3-20 

5-27 

12.40 

23-25 

80 

5-40 

9-OI 

21  .60 

43-25 

90 

10.50 

i8.ii 

IOO 

22.70 

42-54 

Thallium  Alum. 
Gms.  per  ioo  Gms.  H2O. 

A.2T.2(S04),  AlaT^SO,), 

3-15      4-84 
5.86 
7-12 
10-00 


3.80 

4.60 
6.40 

7.60 


14.40 

22  .50 


14-89 

23-57 
38.41 
65.19 


NOTE.  —  Curves  were  plotted  from  the  closely  agreeing  determina- 
tions recorded  by  the  above  named  investigators  and  the  table  con- 
structed from  the  curves. 


AMINES. 


METHYL  AMINE   AND  TRI  METHYL  AMINE,  DISTRIBUTION   BETWEEN 

Water  and  Benzene. 

(Herz  and  Fischer  —  Ber.  38,  1143,  '05.) 

Gms.  N(CHa)3                   Millimols  N(CH3)3 
per  ioo  cc.  per^io  cc. 

Aq.  CgHg 

Layer.        Layer. 

0.584  0.295 

1.377  0.670 

1.819  O.92I 

2.474  1.237 

3.619  1.823 

4.663  2.328 

5.568  2.847 

6.760  3-474 

11.135     5-86i 


Water  and  Amyl  Alcohol. 

(Herz  and  Fischer  —  Ber.  37,  4751,  '04.) 

Gms.  NH2(CH3)             Millimols  NH2(CH3) 
per  ioo  cc.                             per  10  cc. 

Aq. 

Layer. 

o-37 
0.94 

i-57 
1.89 

2.00 

2-53 

3-30 

Alcoholic 
Layer. 

0.12 

o-33 
0-54 
0.69 
0.72 
0.92 
1.24 

Aq. 

Layer. 

I-I5S 
3-036 
5-054 
6.083 
6.429 
8.126 
10.613 

Alcoholic 
Layer. 

0-3804 
1.070 

1-759 

2  .219 

2-3J5 

2.981 

3-974 

Aq. 

CeHe 

Layer. 

Layer. 

o-345 

0.174 

0.812 

0.396 

1-075 

o-545 

i  .462 

0-731 

2.139 

1.077 

2-757 

1.376 

3.292 

1.683 

3-996 

2-053 

6.582 

3-465 

AMINES 


16 


SOLUBILITIES  OP  Di  ETHYL 
AMINE  AND  WATER.* 

(Lattey  —  Phil.  Mag.  [6]  10,  398.  '05-) 


Cms.  NH(C2H6)2 
per  100  Gms. 

t°. 

Aqueous 
Layer. 

Amine 
Layer. 

J55 

21-7 

59-o 

!5<> 

23-6 

55-5 

148 

24-8 

53-5 

146 

26.3 

51.0 

J45 

28.0 

49.0 

144 

31.0 

4S-o 

DISTRIBUTION  OF  TRI  ETHYL  AMINE 
BETWEEN  WATER  AND  AMYL 
ALCOHOL  AT  25°. 

(Herz  and  Fischer — Ber.  37,  4751,  '04.) 


Cms.  N(C2H5)3 
per  ipo  cc. 

Millimols  N(C2H6)., 
per  10  cc. 

Aqueous 
Layer. 

Alcoholic 
Layer. 

Aqueous 
Layer. 

Alcoholic 
Layer. 

0-0885 
0,1683 

0-1866 

0.2502 

2.299 

4-457 
4.922 
6.491 

0-0875 
0.1664 
0.1846 
0.2474 

2.273 
4.408 
4-868 
6.418 

143.5  (crit-  t-)    37-4 


Tri  Ethyl    AMINE 


N(C2H5)3. 
SOLUBILITY  IN  WATER. 

(Rothmund  —  Z.  phys.  Ch.  26,  433,  '98.) 


Gms.  N(C2HB)3  per  100  Gms. 


Gms.  N(C2H6)3  per  100  Gms. 


Aq.  Layer. 

Amine  Layer. 

Aq.  Layer. 

Amine  Layei 

18 

.6  (crit.  temp.) 

51-9 

40 

3-65 

96.48 

20 

14.24 

72.0 

5° 

2.87 

96.4 

25 

7-30 

95.18 

55 

2-57 

96-3 

30 

5.80 

96.60 

60 

2.23 

96-3 

35 

4-58 

96-5 

65 

1.97 

96-3 

SOLUBILITY  OF  TRI  ETHYL  AMINE  IN  MIXTURES  OF  WATER  AND  ETHYL 
ALCOHOL  AT  DIFFERENT  TEMPERATURES.* 

(Meerburg  —  Z.  phys.  Ch.  40,  647,  '02.) 
o%  Alcohol.  13.33%  Alcohol.        28.98%  Alcohol.        38.84%  Alcohol.          60.16%  Alcohol 


G.  N(C2H5] 
t     .        per  100 

t°. 

G.  N(C2H5)3            G.  N(C2H5)3              G.  N(C£fa 
per  100        t°.        per  too           t°.        per  too 

»    "          G.N(C2H6)3 
t  .          per  100 

g.  sol. 

g. 

sol. 

g.  sol. 

g.  sol. 

g.  sol. 

69.2 

1-7 

38-3 

8 

.2 

54 

•5 

22.8 

73 

•4 

31.2 

76-77   71.2 

30.8 

5-6 

13 

9 

45 

.0 

29.8 

65 

•4 

33-3 

74-75     75-o 

23.1 

8-5 

28.0 

21 

.6 

33 

•4 

51  .1 

51 

.6 

40.6 

72-73    80.0 

I8.7 

25-8 

26.4 

30 

.6 

31 

•4 

63-7 

42 

.1 

50.6 

I8.7 

37-2 

24.9 

40 

•5 

30 

•3 

68.5 

40 

•9 

54-7 

19.5 

51.8 

24.2 

49 

.8 

28 

•5 

82.2 

34 

.2 

70.6 

20.5 

68.6 

24.1 

60 

•7 

35 

.0 

91.8 

33 

•  0 

77-5 

20.5 

84.0 

24.0 

69 

•7 

34 

•7 

88.0 

20.5 

89.7 

23-5 

73 

.6 

40 

•5 

9*-3 

21.4 

92.4 

24.0 

81 

•5 

25-8 

95-5 

24.2 

87 

•4 

26.5 

96.1 

25.0 

92 

•  o 

NOTE.  —  Results  for  Tri  Ethyl  Amine,  Water  and  Ethyl  Ether,  and  for 
Tri  Ethyl  Amine,  Water  and  Phenol  are  also  given  by  Meerburg. 

100  gms.  abs.  methyl  alcohol  dissolve  57.5  grams  NH(C6HS)2  at  19.5°. 
100  gms.  abs.  ethyl  alcohol  dissolve  56.0  grams  NH(C6H5)2  at  19.5°. 

(de  Bruyn  —  Z.  phys.  Ch.  10,  784,  1892.) 
*  Determinations  made  by  "  Synthetic  Method,"  see  Note,  page  9. 


i;  AMINES 

SOLUBILITY  OF  Di  PHENYL  AMINE  AND  ALSO  OF  TRI  PHENYL  AMINE  IN 
CARBON  BISULPHIDE. 

(Arctowski  —  Com  pt.  rend.  121,  123,  '95.) 

NH(C6H5)2  in  CS2.  N(C6H6)3  in  CS2. 

AO  Gms.  per   100  .  0  Gms  per  100 

Gms.  Solution.  Gms.  Solution. 

-88J  0.87  -83  1.91 

-117  0.37  -91  1.56 

—  102  1.24 

0.98 


SOLUBILITY  OF  Di  PHENYL  AMINE  IN  HEXANE  AND  IN  CARBON 

BISULPHIDE. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  570,  '94.) 

Gms.  NH(C6H5)2  Gms.  NH(C6H6)2 

0  per  IPO  Gms.  Sol,  in  ;  0  per  100  Gms.  Sol.  in; 

Hexane.  CS2.  Hexane.  CSj.^ 

—  60          ...  1.3  o          2.6        33.7 

—  50  ...  2.2  +IO  3-8  46.8 

—  40  ...  3-8  20  6.7  60.9 

-30        0.5  7-2  30        13.8        76.0' 

—  20        0.8  12.5  40        47-o 

—  10         1.4          21.6  50        94-0          ... 


AMMONIA    NH3. 

SOLUBILITY  OF  AMMONIA  IN  WATER. 

(Roscoe  and  Dittmar  —  Liebig's  Annalen,  112,  334,  '59;  Raoult  —  Ann.  chim.  [5]  I,  262,  '74;  Mallet 

Am.  Ch.  J.  19,  807,  '97.) 

At  760  mm.  Pressure.  At  760  mm.  Pressure. 

G.  NH3          Vol.  NH3  G.NH3       Vol.  NHa 

t°.             per  100  g.           per  i  g.                    t°.  per  100  g.      per  i  g. 

H20.                H20.  H20.             H20 

—  40     294.6      ...          2O  52.6     710 

—  30     278.1      ...          25  46.0     635 

—  20        176.8                              30  40.3        595  (28°) 
~io        111.5                               35  35.5 

o          87.5         1299                40  30.7 

5          77-5         1019                45  27-o 

10          67.9          910                50  22.9          ... 

15          60.0          802                56  18.5 


SOLUBILITY  OF  AMMONIA  IN  AQUEOUS  SALT  SOLUTIONS. 

(Raoult.) 

In  Calcium  Nitrate  Solutions  In  Potassium  Hydroxide  Solutions 

Gms.  NH3  per  100  Gms.  NH3  per  100 

Gms.  Solvent  in:  Gms.  Solvent  in: 

t°.                '  28.38%            In  59-03%  11-25%                25.25% 

Ca(N03)2.        Ca(N03)2.  KOH.                  KOH. 

o     96-25    104.5  72-°     49-5 

8     78.50    84.75  57-o     37-5 

16     65.00    70.5  46-0     28.5 

24      37-3     2I-8 


AMMONIA  18 

MUTUAL  SOLUBILITY  OF  AQUEOUS  AMMONIA  AND  POTASSIUM  CARBON- 
ATE SOLUTIONS. 

(Newth  —  J.  Chem.  Soc.  77,  776,  1900.) 

The  solutions  used  were:  Potassium  Carbonate  saturated  at  15° 
(contained  57.2  grams  K2CO3  per  100  cc.).  Aqueous  Ammonia  of 
0.885  Sp.  Gr.  (contained  about  33  per  cent  ammonia).  The  determina- 
tions were  made  by  adding  successive  small  quantities  of  one  of  the 
solutions  to  a  measured  volume  of  the  other,  and  observing  the  point 
at  which  opalescence  appeared. 

Saturated  KgCOg  in  Aq.  Ammonia.  Aq.  Ammonia  in  Saturated 


t°.        cc.  KaCOs  per          %Ky£O3  Solution  f   cc.  Ammonia        %K2CO3  Solution 

100  cc.  Ammonia.  in  Mixture.  in  100  cc.  KjCOa.       in  Mixture. 

I  2.0  2.0  37-5  72.7 

6  3.0  3.0  47-5  67-6 

ii  5.0  4-7  52-5  65-o 

16  6.5  6.1  60.0  63.0 

21  8.5  8.0  77.5  56.3 

26  10.5  9.5  105.0  49.0 

31  12.5  ii. i  152.5  39.0 

38  20.0  16.6  195-0  33-0 

39  21.0  17-0  220.0  31.0 

42  25.0  20- o  250.0  28.5 

43  35.0  26.0  285.0  26.5 

Above  43°  the  solutions  are  completely  miscible.  If  10  per  cent  of 
water  is  added  to  each  solution  the  temperature  of  complete  miscibility 
is  lowered  to  25°.  The  mutual  solubilities  are: 

Per  cent  K2CO3  Solution  in: 


t°. 

Ammonia 

K2C03  Sol. 

Layer. 

Layer. 

0 

8 

62 

10 

ii 

52 

20 

15 

38 

25  (crit.  pt.) 

25 

With  the  addition  of  12.9  per  cent  of  water  to  each  solution  the 
temperature  of  complete  miscibility  (crit.  pt.)  is  lowered  to  10°.  With 
the  addition  of  18.1  per  cent  water  this  temperature  becomes  o°. 


SOLUBILITY  OF  AMMONIA  IN  ABSOLUTE  ETHYL  ALCOHOL. 

(Delepine  —  J.  pharm.  chim.  [5]  25,  496,  1892;  de  Bruyn  —  Rec.  trav.  chim.  ii,  112,  '92.) 


to 

. 

Cms.  NH3 

Gms.  NH3  per  100  Gms.  Solution. 

Gms.  NH3  per  TOO  Gms.  Alcohol 

. 

Density. 

per  100  cc. 
Solution. 

(Delepine.) 

(de  Bruyn.) 

(Delepine.) 

(de  Bruyn.) 

0 

0.782 

I3-05 

20-95 

19.7 

26.5 

24-5 

5 

0.784 

12  .00 

19.00 

!7-5 

23.0 

21  .2 

10 

0.787 

10.85 

16.43 

15.0 

19.6 

I7.8 

15 

0.789 

9-20 

13.00 

13.2 

15.0 

15.2 

20 

0.791 

7-50 

10.66 

"•5 

II.9 

13.2 

25 

o-794 

6.00 

IO.O 

IO.O 

II  .0 

II  .2 

30 

0.798 

5-15 

9-7 

8.8 

10-7 

9-5 

AMMONIA 


SOLUBILITY  OF  AMMONIA  IN  AQUEOUS  ETHYL  ALCOHOL. 


(Delepine.) 

In  96%  Alcohol. 

In  90%  Alcohol. 

In  8o%j\lcohol. 

t°. 

Sp.  Gr. 

Solution. 

G.  NH3  per 
zoo  Gms.  Sol. 

Sp.  Gr.         G.  NH3  per 
Solution.      100  Gms.  Sol. 

Sp.  Gr.        G.  NH3  per 
Solution.      100  Gms.  Sol. 

O 

0.783 

24-5 

O.8OO            30.25 

0.808        39  -o 

10 

0.803 

18.6 

0.794        28.8 

0.800            28.8 

20 

0.788 

14.8 

0-795             IS'8 

O.82I             19.1 

30 

0.791 

10.7 

0.796             II-4 

0.826            12.2 

In  60%  Alcohol. 


t°. 

Sp.  Gr. 
Solution. 

G.  NH3  per 
100  Gms.  Sol. 

o 

0.830 

50-45 

10 

0.831 

37-3 

20 

0.842 

26.1 

30 

0.846 

21  .2 

In  50%  Alcohol. 


Sp.  Gr. 

Solution. 

0.835 
0-850 
0.869 
0.883 


G.  NH3  per 
100  Gms.  Sol. 

69.77 

43-86 

33-8 

25.2 


SOLUBILITY  OF  AMMONIA  IN  ABSOLUTE  METHYL  ALCOHOL. 

(de  Bruyn  —  Rec.  trav.  chim.  n,  112,  '92.) 

G.  NH3  per  100  Grams. 


O 

5 
10 

15 


G.  NH3  per  100  Grams. 
Solution.         Alcohol. 


29-3 

26.5 

24.2 

21  .6 


41-5 

36-4 
31.8 
27.8 


20 

25 
30 


Solution.         Alcohol. 
19.2  23.8 

20. 0 

16.0 


I6.5 
I4.O 


DISTRIBUTION  OF  AMMONIA  BETWEEN: 
Water  and  Amyl  Alcohol  at  20°.          Water  and  Chloroform  at  20°. 


(Herz  and  Fischer  —  Ber.  37, 
4747,  '04.) 


(Dawson  and  McCrae  —  J.  Ch.  Soc.  79,  496,  '01;  see 
also  Hantsch  and  Sebaldt  —  Z.phys.Ch.so,  258,  '99.) 


Gms  .  NH3  per  TOO  cc. 

G.M.NH3per  IQOCC. 

Gms.NHsper  TOO  cc. 

G.  M.  NH3  per  too  cc. 

Aq.  ^ 

Alcoholic 

Aq. 

Alcoholic 

Aq. 

Crici3 

Aq. 

CrtU3 

Layer 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

o-5 

0 

.072 

O 

•25 

O 

•0035 

O 

.2 

O.OO7 

O.OI 

0-00038 

I  -0 

0 

.147 

O 

•50 

0 

.0073 

O 

•4 

O.OI5 

O-02 

0.00073 

2  -C 

0 

.272 

I 

•  OO 

0 

.0148 

0 

.6 

0.023 

0-03 

O.OOII4 

3-o 

0 

•438 

2 

•  OO 

0 

•0295 

O 

.8 

0.031 

O-O4 

0.00152 

4.0 

0 

•595 

3 

.00 

0 

.0460 

I 

.0 

0-039 

0-05 

0.00193 

5-° 

0 

•756 

I 

.2 

0-046 

O-o6 

O.OO232 

. 

I 

•4 

0-055 

0.08 

o  .  003  i  i 

I 

.6 

0-063 

O-IO 

0-00396 

NOTE.  —  The  influence  of  a  large  number  of  electrolytes  upon  the 
distribution  of  ammonia  between  water  and  chloroform  was  also 
investigated.  For  calculations  of  above  distribution  results,  see  Note, 
page  4. 


AMMONIUM  ARSENATES  20 

SOLUBILITY  OF  AMMONIUM  CALCIUM  ARSENATE  AND  AMMONIUM 
MAGNESIUM  ARSENATE  IN  WATER,  ETC. 

(Field  —  J.  Ch.  Soc.  II,  6,  '73-) 

Grams  per  ioo  Grams  Solvent. 
Solvent. 


Water 0.02  o  014 

Aq.  Ammonia  10%  (Sp.  Gr.  0.88) o.ooi  0.007 

Aq.  NH4C1    5%  .    .    , 0.415 

Aq.  NH4C1  10% 0.095 

AMMONIUM  BENZOATE     NH4C7H6O2. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

Cms.  NH4C7H5O2  per  100  Gms.  Solvent  in : 
t°.  'Water.  Alcohol." 

25  9-52  4-o 

b.  pt.  83.33  13.2 

AMMONIUM    BROMO   PLATINATE     (NH4)2PtBr6. 

100  gms.  sat.  aq.  solution  contain  0.59  gm.  (NH4)2PtBr6  at  20°. 

(Halberstadt  —  Ber.  17,  2965,  '84.) 

AMMONIUM  BROMIDE     NH4Br. 

SOLUBILITY  IN  WATER. 

(Eder  — Abh.  K.  Akad.  Wiss.  (Berlin)  82  ii,  1284,  '80.) 
Gms.  NIL^Br.  per  100  Grams.  Gms.  NH4Br.  per  100  Grams. 

t°.  'Solution.         Water.'  t°.  Solution.  Water. 

10  39.8  66.2  50  48-5  94-3 

20  42.5  74  -o  60  50-2  101.0 

30  44.8  81.3  80  53.5  115-0 

40  46.7  87.5  100  56.1  128.2 

SOLUBILITY  OF  AMMONIUM  BROMIDE  IN  ABSOLUTE  ETHYL  ALCOHOL, 
METHYL  ALCOHOL,  AND  IN  ETHER. 

(Eder;  de  Bruyn  —  Z.  phys.  Ch.  10,  783,  '92.) 

In  Ethyl  Alcohol.  In  Methyl  Alcohol.  In  Ether  (0.729  Sp.  Gr.). 

Gms.  NH4Br  Gms.  NH4Br  Gms.  NILJBr 

per  IPO  prams.  per  100  Grams.  per  100  Grams. 

t°.  Solution.        Alcohol.  Solution.        Alcohol.  Ether. 

15  2-97        3-°6 o-I23 

19  3.12        3.22  ii. i         12.5  

78  9.50       10.50  .... 

Solubility  of  Tetra  Ethyl  AMMONIUM  BROMIDE  N(C2H6)4Br,  and 
of  Tetra  Methyl  Ammonium  Bromide  N(CH3)4Br  in  Acetonitril. 

(Walden  —  Z.  phys.  Ch.  55,  712,  '06.) 

ioo  cc.  sat.  solution  in  CH3CN  contain  9.59  gms.  N(C2H6)4Br  at  25°. 
100  cc.  sat.  solution  in  CH3CN  contain  0.17  gm.  N(CH3)4Br  at  25°. 

AMMONIUM  CADMIUM  BROMIDE  NH4Br.CdBr2.|H2O. 

ioo  parts  of  water  dissolve  137.0  parts  NH4Br.CdBr2.$H2O. 
ioo  parts  of  alcohol  dissolve  18.8  parts  NH4Br.CdBr2.$H2O. 
ioo  parts  of  ether  dissolve  0.36  part  NH4Br.CdBr2.JH2O. 

(Eder  —  Dingier  polyt.  J.  221,  89,  '76.) 


21          AMMONIUM   CARBONATE 
AMMONIUM    CARBONATE    (NH4)2CO3. 

100  grams  H2O  dissolve  100  grams  (NH4)2CO3H2O  at  15°. 
100  grams  glycerine  dissolve  20  grams  (NH4)2CO3  at  15°. 

(Divers  —  J.  Ch.  Soc.  23,  171,  '70.) 


AMMONIUM  BICARBONATE   NH4HCO3. 

SOLUBILITY  IN  WATER. 

(Dibbits  —  J.  pr.  Ch.  [2]  10,  417,  '74.) 

Gms.  NILJICOa  per  100  Grams. 
Solution.          Water. 

10.6 


o 

5 
10 

15 


13.7 
iS-5 


11.9 

T3-7 
15.8 

l8-3 


0       Grams  NHjNCOa  per  100  Grams. 
Solution.          Water. 

20  17-4        21. o 

25  19-3        23.9 

3°  2I-3        27.0 


SOLUBILITY  OF  AMMONIUM  BICARBONATE  IN  AQUEOUS  SOLUTIONS  OF 
AMMONIUM  CHLORIDE  SATURATED  WITH  CO2. 

(Fedotieff  —  Z.  phys.  Ch.  49,  168,  '04.) 


Per  1000  cc.  Solution. 


4.  0              W  I  .  Ol 

1  •      i  cc.  Sol. 

G.M. 

G.M. 

Gms. 

Gms. 

G.  M. 

G.  M. 

Gms 

NH4C1. 

NILJICOs.  NH4C1. 

NHiHCOjj. 

NH4C1. 

OQ 

NH4HC03.  NH4C1. 
1.22            ^   ^ 

NH4HCOa. 

T  T  f\      ^v 

.     .     • 

o     1.077 

4.41 

o-37 

235 

•9 

29 

.2 

•  \J 

5-42 

0.46 

290.8 

i  iy  .  o 

36.0 

15       1.064 

O-O 

2  .12 

0 

•  o 

I67 

.2 

o.o 

2.36 

o.o 

186.4 

15       1.063            0-5 

1.84 

26 

.8 

145 

.2 

0.56 

2.06 

29.9 

162.9 

15       1.062 

1.0 

i-59 

53 

•5 

125 

•5 

1  .13 

1.  80 

60.6 

142.2 

15       1.062 

1.41 

1.42 

75 

•4 

112 

.2 

i-59 

I  .60 

85.1 

126.9 

IS 

.065 

1,89 

4.28 

100 

.8 

101 

.1 

2.18 

1.48 

116.8 

II6.8 

15 

.069 

2.87 

0.99 

153 

•3 

78 

.2 

3-42 

1.18 

183.0 

93-3 

IS 

.076 

3-84 

0.79 

205 

.2 

62 

•5 

5-03 

0.98 

269.3 

77-3 

.085 

4.82 

0.65 

257 

•9 

51 

•4 

6.21 

0.84 

332.5 

66.4 

15 

.085 

4-95 

0.62 

264 

.8 

48 

•9 

6.40 

0.81 

343-5 

64.2 

30 

o.o 

3-42 

o.o 

270.0 

7O 

*7  .A 

T  .  TC 

•20*7  .n 

nr  .r» 

SOLUBILITY  OF  AMMONIUM  BICARBONATE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  BICARBONATE  SATURATED  WITH  CO2. 

(Fedotieff.) 


o 

o 

15 
15 


Per  1000  cc.  Solution. 


Wt.of      'r    M 
i  cc.  Sol.  NGHM6g 

G.M. 

Gms. 
i.  NaHCO3. 

Gms. 

'  I 

.072 

0 

•53 

1.28 

44.6 

IOI 

•4 

I 

.064 

0 

.0 

2  .12 

o.o 

I67 

.2 

I 

•  090 

o 

•63 

1.92 

52-5 

I5! 

•3 

Per  looo  Grams 


G.M. 
NaHCOjj. 

O.O 
0.58 
0.0 
0.71 

o.o 

0.83 


G.M. 


1.51 

i-39 
2.36 
2.16 
3-42 
2.91 


Gms. 
aHC03. 

0-0 
48.2 

o.o 
59-2 

o.o 
70.0 


Gms. 


119.0 
109.4 
186.4 
170.6 
270.0 
230.0 


AMMONIUM  BICARBONATE     22 

SOLUBILITY    OF    MIXTURES    OF    AMMONIUM    BICARBONATE,    SODIUM 
BICARBONATE,  AND  AMMONIUM  CHLORIDE  IN  WATER 
SATURATED  WITH  CO2. 

(Fedotieff.) 


to         Wt.  of 

Gram  Mols.  per  1000 
Gms.  H2O. 

Gms.  per  1000  Gms.  H2O. 

Solid 

Phase 

i  cc.  Sol 

"    NaHCO3. 

NaCl. 

NH4C1. 

NaHCO3. 

NaCl. 

NI^Cl. 

iruasc. 

o 

.114 

o-59 

0.96 

4 

.92 

49.61 

56 

.16 

263 

•4 

a+b  +  c 

O 

.187 

0-12 

4-83 

2 

•74 

IO.O9 

282 

.6 

146 

•7 

" 

15 

.116 

o-93 

0.51 

6 

.28 

78.18 

29 

.84 

336 

.2 

u 

15 

.I78 

0.18 

4.44 

3 

•73 

15.13 

259 

.8 

199 

.6 

14 

15 

0.30 

3-09 

4 

•56 

25.22 

180 

.8 

244 

.1 

a  +  c 

15 

.128 

0.51 

1.68 

5 

•45 

42.87 

98 

.28 

291 

•7 

" 

15       1.  112 

0.99 

o-35 

5 

•65 

83.22 

20 

•47 

302 

•4 

a  +  b 

15       I.IOS 

1.07 

O.2O 

5 

.21 

89.95 

II 

.70 

278 

•9 

a 

15     1.106 

I  .12 

o.n 

4 

.92 

94.14 

6 

•44 

263 

•4 

a 

15     i.ioi 

1.16 

0.14 

4 

.00 

97-52 

8 

.19 

214 

.i 

(i 

15     1.090 

o-93 

o-95 

2 

•03 

78.18 

55 

•58 

108 

.6 

(( 

a  = 

NaHCO3 

, 

b  = 

NH4HCO3, 

c 

= 

NH4C1. 

AMMONIUM    URANYL    CARBONATE     2(NH4)2CO3UO2CO3. 

(Ebelmen.) 

100  grams  H2O  dissolve  5  grams  of  the  salt  at  15°. 


AMMONIUM    LEAD    COBALTICYANIDE     NH4PbCo(CN)6.3H2O. 

(Schuler  —  Sitz.  Ber.  K.  Akad.  W.  (Berlin)  79,  302.) 

ioo  grams  H2O  dissolve  12.0  grams  of  the  salt  at  18°. 


AMMONIUM    CHLORIDE     NH4C1. 

SOLUBILITY  IN  WATER. 

(Mulder;  below  o°,  Meerburg  —  Z.  anorg.  Ch.  37,  203,  1903.) 

Gms.  NH4C1  per  ioo  Gms.                                 Gms.  NH4C1  per  ioo  Gms. 

Solution.          Water."                                             Solution.  Water". 

-15             19.7         24.5  40            31.4  45-8 

-10.9        20.3         25.5  50            33.5  50.4 

-5.7          21.7         27.7  60            35.6  55.2 

o            22.7         29.4  70            37.6  60.2 

+  5            23.8        31.2  80            39.6  65.6 

10            24.9        33.3  90            41.6  71.3 

15            26.0        35.2  ioo            43 -6  77-3 

20            27.1        37-2  no            45-6  83.8 

25            28.2        39.3  115.6        46.6  87.3 

30  29.3        41.4 

Density  of  saturated  solution  at  o°  =  1.088,  at  15°  =  1.077,  at  I9° 
-  1-075- 


AMMONIUM  CHLORIDE 


SOLUBILITY   OF  AMMONIUM   CHLORIDE   IN   AQUEOUS   AMMONIUM   BI- 
CARBONATE SOLUTIONS  SATURATED  WITH  CO2. 

(Fedotieff  —  Z.  phys.  Ch.  49,  169,  1904.) 


Per  1000  cc.  Solution. 


Per  1000  Cms.  H2O. 


t°. 

VV  I  .   Ol 

i  cc.  Sol. 

G.M. 

G.  M. 

Gms. 

Gms. 

G. 

M. 

G.  M. 

Gms. 

Gms. 

NH4HCO3.  NH4C1.  NH.HCC 

•3.  NKiCl. 

NH.HCG-3.  NH/C1. 

NH4HC1.  NH4C1. 

0 

1  .069 

O-O 

4.60 

O-O 

246 

.1 

O 

•  O 

5-57 

o.o 

298.0 

0 

1.077 

o-37 

4.41 

29.2 

235 

9 

O 

.46 

5-42 

36-0 

290.8 

15 

1.077 

o.o 

5-29 

o.o 

283 

.1 

O 

•  0 

6.64 

o.o 

355-o 

1.085 

0.62 

4-95 

48.9 

264 

.8 

O 

.8l 

6.40 

64.2 

343-5 

30 

O 

•  O 

7.78 

o.o 

416.4 

70 

I 

7  .A.Q 

OT  .0 

70*7  .0 

SOLUBILITY    OF   AMMONIUM    CHLORIDE    IN    AQUEOUS    SOLUTIONS    OF 
SODIUM  CHLORIDE  SATURATED  WITH  CO2. 

(Fedotieff.) 


Per  1000  cc.  Solution. 


Per  1000  Gms.  H2O. 


t°. 

Wt.of 

G. 

M. 

G.  M. 

Gms. 

Gms. 

G.  M. 

G.  M. 

Gms. 

Gms. 

i  cc.  Sol. 

NaCl. 

NH4C1. 

NaCl. 

NH4C1. 

NaCl. 

NH4C1. 

NaCl. 

NH4C1. 

0 

I  .069 

O 

.0 

4.60 

O 

.0 

246.1 

0-0 

5-57 

o.o 

2Q8.0 

O 

1.085 

4 

.04 

2.26 

236 

.5 

121  -O 

4.89 

2-73 

286.4 

146.1 

15 

1.077 

0 

.0 

5-29 

O 

•  o 

283-1 

O-O 

6.64 

o.o 

355-o 

15 

1.097 

o 

.81 

4.71 

47 

•5 

252.1 

I  .02 

5-91 

59-8 

316.4 

15 

I  .I2O 

I 

.68 

4-13 

98 

•  o 

221  .7 

2.09 

5.18 

122  .4 

277.0 

15 

I-I53 

2 

-87 

3-38 

168 

•  o 

180.7 

3-57 

4.20 

208.9 

224.7 

15 

I-I75 

3 

•65 

2.98 

213 

•5 

159-4 

4-55 

3-72 

266.8 

198.8 

30 

o-o 

7.78 

0-0 

416.4 

30 

1.166 

3 

•30 

3-70 

J93 

•  o 

198.0 

4.26 

4-77 

249-0 

255-4 

45 

O-O 

9-03 

0-0 

483.7 

AC 

A.O 

6.02 

277  .0 

722.1 

SOLUBILITY    OF   AMMONIUM    CHLORIDE    IN    AQUEOUS    SOLUTIONS    OF 
HYDROCHLORIC  ACID  AT  o°. 

(Engel  —  Ann.  chim.  phys.  [6]  13,  379,  '88.) 


Sp.  Gr.  of 

Solutions. 


•  076 
.069 
.070 
.071 

•073 
.078 


I 
I 
I 

I 
I 
I 

I  .100 

1.114 


Milligram  Molecules  per                        Grams  per  100  cc. 
10  cc.  Solution.                                          Solution. 

HCl. 

NH4C1. 

HCl. 

NH4C1. 

O-O 

46.12 

o.o 

24.61 

2.9 

43  -6 

1.05 

23  -16 

5-5 

41  -o 

1.99 

21.78 

7-85 

39-15 

2.84 

20.79 

10.85 

36-45 

3-93 

19.36 

21.4 

27-37 

7-74 

14-54 

53-o 

10.87 

19.18 

5-78 

61  .0 

8.8 

22  .07 

4.67 

Sat.  HCl  at  1  2° 

3  -7  at 

17° 

AMMONIUM  CHLORIDE 


24 


SOLUBILITY  IN  AQUEOUS  AMMONIA  SOLUTIONS 

(Engel  —  Bull.  soc.  chim.  [3]  6,  17,  1891.) 

AT    0°. 

Sp.  Gr.  of 

Milligram 
per  10  cc. 

Molecules 

Solution. 

Grams  per  100  cc. 
Solution. 

Solutions. 

'NH3. 

NI^Cl. 

NH4OH. 

NH4C1. 

1.067 

5-37 

45-8 

0.92 

24.52 

1.054 

12.  02 

45-5 

2.05 

24-35 

I.03I 

38.0 

44-5 

6.48 

23-82 

I  .025 

47-o 

44.0 

8.02 

23-56 

I.OI7 

54-5 

43-63 

9-30 

23-35 

o-993 

80.0 

43.12 

13.66 

23.09 

0.992 

90.0 

44.0 

I5-36 

23-56 

0.983 

95-5 

44-37 

16.29 

23-75 

o-953 

130.0 

49-75 

22.18 

26.63 

0.931 

169-75 

60-0 

28.97 

32.14 

SOLUBILITIES  OF  MIXTURES  OF  AMMONIUM  CHLORIDE  AND  OTHER  SALTS 

IN  WATER. 

(Riidorff,  Karsten,  Mulder.) 

Both  salts  present  in  solid  phase. 

4,0>  Grams  per  100  Grams  H2O. 

b.pt.    67.7NH4Cl+2i.9KCl     M 


te. 
19. 

21. 

20. 

18. 

15- 

22. 

5 

5 

o 

5 

0 
0 

( 

jrams  ] 

Der  K 

30   (Jl 

•an 

is  tiz^J 

R 
R 
R 
K 
R 
R 

29. 
26. 

33- 
39- 
28. 

30- 

2 

8 
8 

2 

9 
4 

NH4Cl+i74.o 
"     +   46-5 
"     +    ii.  6 
"     +    17.0 
"     +    16.9 
"      4-    19.1 

NH4NO3 

(NH4)2S04 
BaCl2 
Ba(N03)2 
KC1 
KC1 

14.8  38.8 

18-5  39-8 

14.0  36.8 

18.7  37.9 

18.7  22.9 


+  34.2KN03K 
+  38.6KNO3K 
+  14.1  K2SO4R 
+  i3.3K2S04K 
R 


SOLUBILITY  OF  AMMONIUM  CHLORIDE  IN  ABSOLUTE  ETHYL  AND  METHYL 
ALCOHOL  AT  19°  AND  IN  AQUEOUS  ETHYL  ALCOHOL 
SOLUTIONS. 

100  grams  absolute    ethyl    alcohol  dissolve  0.62  grams  NH4C1. 
100  grams  absolute  methyl  alcohol  dissolve  3.35  grams  NH4C1. 

(de  Bruyn  —  Rec.  trav  chim.  n,  156,  '92.) 


In  Aqueous  Alcohol  at  30°. 

(Bathrick  — J.  Physic.  Chem.  i,  159,  '96.) 


Wt.  per  cent 
Alcohol. 

per  100  g. 
Alcohol. 

Wt.  per  cent 
Alcohol. 

G.  NH4C1 
per  100  g. 
Alcohol. 

O 

40.4 

45-9 

17.0 

8-3 

35-3 

54-3 

I4.O 

l6.9 

31.8 

65  -o 

9.6 

25-9 

27-5 

75-6 

6.4 

34-4 

21.7 

87.9 

2-9 

In  Aq.  Alcohol  of  45  Wt.  %. 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  147,  '65.) 


' 

G.  NH4C1 

t°. 

per  100  g. 
Alcohol. 

4 

II  -2 

8 

12.6 

27 
38 
56 

19.4 
23.6 
30.1 

25  AMMONIUM  CHLORIDE 

SOLUBILITY  OF  AMMONIUM  CHLORIDE  IN  AQUEOUS  GLYCERINE  SOLU- 
TIONS AND  IN  AQUEOUS  ACETONE  SOLUTIONS  AT  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  45,  263,  267,  '05.) 


In  Aqueous  Glycerine. 

(Sp.  Gr.  of  Glycerine  1.255,  Impurity  about  1.5%.) 


In  Aqueous  Acetone. 


Wt.% 

NH4C1  per  100  cc.           Sp.  Gr. 
Solution.                      ,    2s°               Vol.% 

NH4C1  per  100  cc. 

Solution. 

Sp.  Gr. 

Glycerine* 

Millimols. 

Grams.                    4° 

Millimolb 

Grams.             ""*  4° 

0 

. 

585 

.1 

3I-32 

•0793 

0 

585 

I 

31 

•32 

1.0793 

13 

.28 

544 

.6 

29.16 

.0947 

10 

534 

I 

28 

•59 

I.  O6l8 

25 

.98 

502 

•9 

26.93 

.1127 

20 

464 

6 

24 

.87 

I.045I 

45 

•36 

434 

•4 

23  .26 

.1452 

30 

396 

7 

21 

•23 

1.0263 

54 

•23 

403 

•5 

21  .60 

.1606 

40 

328 

5 

17 

•59 

o  .  9998 

83 

.84 

291 

•4 

15.60 

.2225 

^46.5 

L    283 

7 

o  .  9800 

100 

.00 

228 

•4 

12.23 

.2617 

^85-7 

U      18 

9 

I 

.01 

0.8390 

90 

9 

4 

O 

•5o 

0-8274 

* 

Between  these  two  concentrations  of  acetone,  the 

solution 

separates  into 

two  layers. 

L  indicates 

lower  layer,  U  indicates  "upper  layer. 

Solubility  of  Tetra  Ethyl  AMMONIUM  CHLORIDE  N(C2H6)4C1,  and 
also  of  Tetra  Methyl  Ammonium  Chloride  N(CH3)4C1  in  Acetonitril. 

100  cc.  sat.  solution  in  CH3CN  contain  29.31  gms.  N(C2H6)4C1  at  25°. 
100  cc.  sat.  solution  in  CH3CN  contain  0.265  gms-  N(CH3)4C1  at  25°. 

(Walden  — Z.  physik.  Chem.  55,  712,  '06.) 


AMMONIUM 


CHROMATES. 

SOLUBILITY  IN  WATER 


AT  30' 


(Schreinemaker  —  Z.  physic.  Chem.  55,  89,  '06.) 
Composition  in  Wt.  per  cent  of: 

Solid  Phase. 


The  Solution. 

The  Residue. 

%  Cr03. 

%  NH3. 

%  Cr03. 

%  NH3. 

6-933 

22.23 

.  .  . 

9.966 

16.53 

47-59 

20-44 

16.973 

8.20 

22-53 

6-37 

38-03 

12.15 

27.09 

6.87 

48  .02 

12  .01 

26.19 

5-7o 

47  -38 

8.81 

25-99 

5.10 

41.56 

7-58 

30.16 

3-5o 

38.89 

3.10 

61.08 

8.80 

42.44 

3-i5 

59-72 

6-75 

44-08 

2.27 

54-90 

4.14 

52.91 

i  .11 

60.88 

3-09 

54-56 

1.03 

63.07 

3-°9 

56-57 

0.97 

65.70 

2-95 

58-87 

0.65 

69.74 

3-24 

62.48 

0.46 

71-93 

3.10 

63.60 

o  .40 

73-68 

1.18 

63.66 

0.41 

71  .47 

2.07 

62.94 

0-21 

62.28 

o.o 

.  .  . 

(NH4)2CrO< 


(NH4)2Cr04+(NH4)2Cr207 
(NH4)2Cr207 


(NH4)2Cr207+(NH4)2Cr301(, 
(NH4)2Cr3O10 

(NH4)2Cr3010  +  (NH4)2Cr4013 
(NH4)2Cr403 


(NH4)2Cr4O13+CrO3 

U 

Cr03 
CrOs 

100  gms.  of  the  sat.  aq.  solution  contain  28.80  gms.(NH4)2CrO4  at  30 
100  gms.  of  the  sat.  aq.  solution  contain  3  2. 05  gms.  (NH4)2Cr2O7at  30 


AMMONIUM    FLUOBORIDE 


26 


AMMONIUM  FLUOBORIDE   NH43BF3, 

100  parts  of  water  dissolve  25  parts  salt  at  16°,  and  about  97  parts 

at  b.  pt.  (Stolba  —  Chem.  Techn.  Cent.  Anz.  7,  459-> 


AMMONIUM  FORMATE 

Formate. 


HCOONH4,    and   also    Ammonium    Acid 


SOLUBILITY  IN  WATER. 

(Groschuff  —  Ber.  36,  4351,  '03.) 


Solid. 


—  20 
o 

20 
40 
60 
80 


Gms.  HCOONH4 
per  100  Gms. 

Solution.  Water. 

41.9      72    HCOONH, 

50.5       102 


58.9 
67.I 

75-7 
84.2 
116  f.  pt. 


143 
204 

3" 


Gms.  per  100  Gms. 
t°.                   Solution. 

Solid. 

PV.OCO 

HCOONH2  +  HCOOH.                *  ""~" 

6-5 

46.7 

34-1 

HCOONH4.HCOOH 

i-5 

49.6 

36.2 

M 

6.0 

5J-3 

37-4 

11 

8-5 

52-1 

38.0 

M 

7 

49.6 

36.2 

HCOONH4  labil. 

i3 

53-° 

38.6 

"           stabil. 

29 

55-8 

40.7 

«               « 

39 

57-8 

42.2 

H2O  free  solution. 

SOLUBILITY  OF  AMMONIUM  FORMATE  IN  FORMIC  ACID  SOLUTIONS. 

(Groschuff.) 

30  grams  of  HCOONH4  dissolved  in  weighed  amounts  of  formic  acid 
and  cooled  to  the  point  at  which  a  solid  phase  separated. 

G.  M. 
COONI 

per 


Gms. 

G.  M. 

Gms. 

HCOONH*  HCOONH4         qni;H 

HCOONH, 

t°. 

per 
100  Gms. 

per 
100  G.M. 

Phase. 

t°. 

per 
100  Gms 

Solution. 

HCOOH. 

Solution 

-  3 

35-3 

39-9 

HCOONH 

v  " 

50.0 

HCOOH 

39 

57.8 

+  8.5 

40.6 

49.9 

11 

78 

73-i 

21.5 

50.0 

73-° 

" 

116  m.pt. 

,   IOO.O 

Solid 
Phase. 


73.0     HCOONH,  labil. 
loo.o  stabil. 

199.0 

00 


AMMONIUM  IODATE  NH4IO3. 

100  parts  H2O  dissolve  2.6  parts  salt  at  15°  and  14.5  parts  at  100°. 

(Rammelsberg  —  Pogg.  Ann.  44,  555,  1838.) 

Tetra  Methyl  AMMONIUM  IODIDE  N(CH3)J. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Walden  —  Z.  physik.  Chem.  55,  708,  '06.) 


SD 

Gr.  of 

Gms.  N(CH3)4  I  per  100. 

Solvent. 

Formula. 

t  °. 

£' 

Gi 

us. 

cc 

,  Solution. 

Solution. 

Water 

H20 

O 

I 

-Ol88 

2 

•  OI 

I 

•97 

Water 

H2O 

25 

I 

.0155 

5 

.31-5  .89 

>5 

.22 

Methyl  Alcohol 

CH3OH 

o 

O 

.8025 

o 

.l8-0.22 

o 

.22 

Methyl  Alcohol 

CH3OH 

25 

0 

-7920 

0.38-0.42 

o 

.48 

Ethyl  Alcohol 

C2H5OH 

25 

0 

.7894 

o 

.09 

Glycol 

(CH2OH) 

2 

o 

J 

.OI4 

Glycol 

(CH2OH) 

3 

25 

I 

.0678 

0 

.240 

0 

.224 

Acetonitril 

CH3CN 

25 

.  .  . 

o 

.650 

Nitro  Methane 

CH3N02 

o 

I 

•1387 

o 

.25-0-32 

o 

.22 

Nitro  Methane 

CH3NO2 

25 

I 

.1285 

o 

.34-0.38 

0 

.21 

Acetone 

(CH3)2CO 

0 

0 

,118 

.  . 

Acetone 

(CH3)2CO 

25 

o 

.187 

Salicyl  Aldehyde 

C6H4.OH. 

COH 

o 

I 

.1492 

o 

.302 

o 

.263 

Salicyl  Aldehyde 

CJL.OH. 

COH 

25 

I 

•1379 

o 

.510 

o 

,484 

27  AMMONIUM  IODIDE 

Tetra  Ethyl  AMMONIUM  IODIDE    N(C2H6)J. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Walden  — Z.  physik.  Chem.  55,  6gS,  '06.) 


SD  Gr  of 

Gms.  N(C2H5)4  I  per  100. 

Solvent. 

Formula. 

t°. 

Solution. 

cc.  Solution.        Sohitkm 

Water 

H2O 

o 

I  .0470 

16.31 

I5-58 

Water 

H2O 

25 

I  .IO2I 

36.33(35 

•5)  J3-44 

Methyl  Alcohol 

CH3OH 

o 

0.8326 

3-7-4-3 

4-44 

Methyl  Alcohol 

CHsOH 

25 

o  .  8463 

10.5  (10 

.7)  12.29 

Ethyl  Alcohol 

C2H5OH 

0 

0.7928 

0.348 

0-439 

Ethyl  Alcohol 

C2H5OH 

25 

0.7844 

0.98  (o 

.88)  1.249 

Glycol 

(CH2OH)2 

0 

I  .  1039 

3-27 

2-97 

Glycol 

(CH2OH)2 

25 

I  .  0904 

7-63  (7 

•55)  7-oo 

Acetonitril 

CH3CN 

0 

0.8163 

2.24 

2.74 

Acetonitril 

CH3CN 

25 

0.7929 

3-o4(3 

•54)  3-83 

Propionitril 

CH3CH2CN 

0 

0.8059 

0.618 

0.767 

Propionitril 

CH3CH2CN 

25 

0.7830 

0.81-1. 

01     1.29 

Benzonitril 

C6H5CN 

25 

.  .  . 

0.467 

.  .  . 

Methyl  Sulphocyanide 

CH3SCN 

25 

1.0828 

4.40 

4.06 

Ethyl  Sulphocyanide 

C,H5SCN 

25 

I  .0012 

0-475 

0-47 

Nitro  Methane 

CH3NO2 

o 

1.1658 

3-59 

3.004 

Nitro  Methane 

CH3N02 

25 

I.I476 

5.61-6. 

27     5-6i 

Nitroso  Dimethylin 

(CH3)2N.NO 

25 

I  .OO59 

2.67 

2.66 

Acetyl  Acetone 

CH3COCH2COOCH3 

25 

0.268 

Furfurol 

C4H3O.COH 

o 

I.I738 

3-91 

3-33 

Furfurol 

C4H3O.COH 

25 

I  .1692 

5-33 

4-55 

Benzaldehyde 

C0H5COH 

25 

o-43 

Salicylaldehyde 

C6H4.OH.COH 

25 

change- 

able-i7 

.7 

Anisaldehyde 

C6H4.OCH3.COH 

25 

o-59 

Acetone 

(CH3)2CO 

0 

0.7991 

0.174 

0.218 

Acetone 

(CH3)3CO 

25 

0.249 

0.218 

Ethyl  Acetate 

CH3COOC2H5 

25 

0.00039 

Ethyl  Nitrate 

C2H5ON02 

25 

I  .0984 

0.062 

0.056 

Benzoyl  Ethyl  Acetate 

C6H5COCH2COOC2H5  25 

I  •  I3C3 

0.321 

0.284 

Di-Methyl  Malonate 

CH,(COOCH3)2 

25 

I  .  1335 

0.040 

0-035 

Methyl  Cyan  Acetate 

CH2CNCOOCH3 

o 

I  .1341 

1.82 

1.605 

Methyl  Cyan  Acetate 

CH2CNCOOCH3 

25 

2-83 

Ethyl  Cyan  Acetate 

CH2CNCOOC2H5 

0 

1.0760 

i-o57 

0.981 

Ethyl  Cyan  Acetate 

CH2CNCOOC2H6 

25 

I  .0607 

1.71 

1.41 

AMMONIUM    IODIDE 


28 


Tetra  Propyl  AMMONIUM  IODIDE     N(C3H7)4I. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Walden  —  Z.  phyaik.  Chem.  55.  700.  '06.) 

Gms.  N(C3H7)4  I  per  100. 
cc.  Solution. 


Solvent. 


Formula. 


Sp.  Gr.  of 
Solution. 


Gms. 
Solution. 


Methyl  Alcohol 

CH3OH 

o 

0 

•9756 

40 

.92 

41 

•94 

Methyl  Alcohol 

CH3OH 

25 

I 

.0187 

56 

.42 

55 

•37 

Ethyl  Alcohol 

C2H8OH 

o 

0 

•8349 

6 

.5-6.8 

8 

.14 

Ethyl  Alcohol 

C2H5OH 

25 

0 

.8716 

19 

.88-20.29 

23 

.28 

Acetonitril 

CH3CN 

o 

0 

•8553 

13 

•03 

15 

.24 

Acetonitril 

CH3CN 

25 

0 

.8584 

18 

.69 

21 

•77 

Propionitril 

C2H6CN 

o 

o 

.8280 

6 

•37 

7 

.66 

Propionitril 

C-jHjsCN 

25 

0 

.8191 

9 

•65 

ii 

.76 

Benzonitril 

C6H6CN 

25 

.0199 

8 

•44 

8 

•35 

Nitro  Methane 

CH3NOa 

o 

.181 

14 

•79 

12 

•52 

Nitro  Methane 

CH3N02 

25 

.158 

22 

.24 

19 

.21 

Nitro  Benzol 

C6H6N02 

25 

'  5 

.71 

4 

•79 

Benzaldehyde 

C6H6COH 

o 

.0581 

7 

.06 

6 

.67 

Benzaldehyde 

CeHsCOH 

25 

•0549 

9 

.87 

9 

•35 

Anisaldehyde 

C6Hfi.OCH3.COH 

0 

.1114 

5 

.60 

5 

.04 

Anisaldehyde 

C6H6.OCH3.COH 

25 

I 

.1004 

6 

•75 

6 

.14 

Salicylaldehyde 

C6H5.OH.COH 

52 

.  .  . 

39 

.28 

Ethylnitrite 

C6H6ONO8 

o 

I 

.1207 

0 

•522 

o 

.466 

Ethylnitrite 

C6H5ON02 

25 

I 

.1025 

o 

•653 

o 

•592 

Di-Methyl  Malonate 

CH2(COOCH3)2 

o 

I 

•I532 

o 

.298 

o 

•259 

Di-Methyl  Malonate 

CH2(COOCH3)2 

25 

I 

•1345 

o 

.320 

o 

.282 

Acetone 

(CH3)2C 

o 

o 

.8259 

2 

.692 

3 

.26 

Acetone 

(CH3)2CO 

25 

0 

.8049 

3 

•944 

4 

.90 

Ethyl  Acetate 

CHaCOOCA 

25 

0 

•8975 

o 

.0063 

o 

.007 

AMMONIUM     NITRATE    NH4NO3. 

SOLUBILITY  IN  WATER. 

(Schwarz  —  Ostwald's  Lehrbuch,  ad  ed.  p.  425;  Muller  and  Kaufmann  —  Z.  physik.  Chem. 
42,  497,  'oi-'oz.) 


t° 

Sp.  Gr. 
Solution. 

G.  Mols. 
NH4NO3  per 
too  Mols.  H2C 

Gms.  NH4NO3  per 
)ioo  Gms. 

Solid 
Phase. 

•   Solution. 

Water. 

o 

.  .  . 

26 

•63 

54 

.19 

118 

•3 

NH4NO3  rhomb,  ft 

12 

.2 

•  2945 

34 

•5o 

60 

•53 

J53 

•4 

« 

20 

.2 

.3116 

43 

30 

65 

.80 

192 

•4 

it 

25 

•  O 

•3*97 

48 

19 

68 

•i7 

214 

.2 

H 

30 

.O 

•3299 

54 

40 

70 

•73 

241 

.8 

tc 

32 

.  j 

•3344 

57 

.60 

7i 

97 

256 

•9 

NH4NO3 

rhomb,  ft  +  rhomb,  a 

35 

.0 

•3394 

59 

.80 

72 

.64 

265 

.8 

NH4N03 

rhomb,  a 

40 

.0 

•3464 

66 

.80 

74 

.82 

297 

.0 

« 

50 

.0 

77 

.41 

77 

•49 

344 

.0 

M 

60 

.0 

94 

•73 

80 

.81 

421 

.0 

(( 

70 

.0 

112 

•30 

83-32 

499 

.0 

« 

80 

.0 

130 

•50 

85 

•25 

580 

.0 

It 

90 

.0        ... 

166 

•5o 

88 

.08 

740 

.0 

NH4NO3 

rhombohedral  ? 

100 

.0 

196 

.00 

89 

•7i 

871 

.0 

« 

a9  AMMONIUM  NITRATE 

SOLUBILITIES  OF  MIXTURES  OF  AMMONIUM  NITRATE  AND  OTHER 

SALTS. 

(Riidorff  — Mulder.) 

ioo  gms.  H2O  dissolve  162.9  gms.  NH4NO3  +  77.1  gms.  NaNO,  at 
i6°R. 

ioo  gms.  H2O  dissolve  88.8  gms.  NH4NO3  +  40.6  gms.  KNO,  at 
9°  M. 

ioo  gms.  H2O  dissolve  101.3  gms.  NH4NO3  +  6.2  gms.  Ba(NO8)2  at 
9°M. 

SOLUBILITY  OF  AMMONIUM  NITRATE  IN  AMMONIA. 

(Kuriloff  —  Z.  physik.  Chem.  25,  109,  '98.) 

Mols.  NH4NO8 

Gms.  Gms.          per  ioo  Mols.  Gms. 

NH4NO3  t°. 

+  NH3. 

o.o  33.3 

6-25  35-9 

1.2457  13.9  68.8 

0.3700  32.3  94.0 

o-35J5  36-9  J9o-8 

0.2607  38.3  168.0 


-80 
-60 

-44-5 
-30 
-10.5 
o 


Gms. 
NH3. 

IOO 


I.39I8 
0.9526 
0.8308 
0.9675 

o  -  7600 


0-9358 
0.7746 
4.2615 
0.6439 
0.7578 


Mols. 

Gms.      per  ioo 

NH3.  N^NOs 

+  NHs? 


0.2352 
0.1857 

0-7747 
0.0665 

0.0588 


45-9 
47-o 
53-8 

67-3 
74.2 

100.0 


t°  =  temperature  of  equilibrium  between  solution  and  solid  phase. 
SOLUBILITY  OF  AMMONIUM  NITRATE  IN  NITRIC  ACID. 

(Groschuff  — Ber.  37,  1488,  '04.) 


Determinations  by  the  "  Synthetic  Method,"  see  Note,  page  9. 

Gms.            Mols.                                                             Gms.          Mols. 
to            NHiNOa     NHiNOs                Solid                 to       NH4NO3      NH4NO3              Solid 
'            per  ioo         per  ioo                Phase.                              per  ioo        per  ioo               Phase. 
Gms.  Sol.  Mols.  HNO3.                                                 Gms.  Sol.  Mols.  HNO3. 

8 

21.  I 

21 

.1 

N^NOs-aHNOg 

II 

.0 

51-7 

84- 

3        NH.NOs.HNOs 

23 

28.7 

31 

.6 

a 

12 

.0 

54.7 

95- 

I 

"        labil. 

29 

.5m.pt. 

38.8 

5o 

.0 

" 

II 

•5 

57-6 

108.0 

b 

27 

•  5 

44.6 

63 

.4 

b 

II 

•  5 

54-0 

92. 

4      N 

r^NOs     labil. 

23 

•5 

49-4 

76 

.8 

" 

17 

.0 

54-7 

95- 

I 

44      stahU. 

17 

•  5 

54-o 

92 

•  4 

" 

27 

.0 

56.2 

IOI. 

0 

44 

16 

4 

•5 
.0 

54-3 
45-8 

93 
66 

•  5 
•7 

NH4NO3.HN03 
labil 

49 
79 

.0 
.0 

60.4 
68.1 

120.0 

168.0 

a=  solution  in  HNO3,        b  =  solution  in  NH,NOj 


SOLUBILITY  OF  AMMONIUM  TRI-NITRATE  IN  WATER. 

(Groschuff.) 


Gms.  NH4NO3 

Gms.  HNO3 

Mols.  NH4NO8*  Mols. 

t°. 

per  ioo 
Gms. 

per  ioo 
Gms. 

per  ioo 
Mols. 

pel 
total 

Solution. 

Solution. 

H2O. 

Solt 

-8 

34-2 

53-9 

64.3 

22 

-2.5 

34-8 

54-8 

75-1 

23 

35-4 

55-8 

9O.O 

24 

i'-s 

36.6 

56-9 

113  .O 

25 

19-5 

37-4 

58.9 

225.0 

29 

25.0 

38.1 

60.0 

450.0 

31 

29.5  m.  pt. 

38.8 

61.2 

o.o 

O 

Solid 

Mols.  Phase 

tion. 

o     NHJSTOs^HNO, 

i 

•3 
•7 
.o 
.o 


or  NH*NO8.2HNO8. 


AMMONIUM    NITRATE  30 

SOLUBILITY  OF  AMMONIUM  NITRATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Fleckenstein  —  Physic.  Z.  6,  419,  '05.) 
Grams  of  NH4NO3  Dissolved  per  100  Grams  Aq.  Alcohol  of  (Wt.%). 


f~. 

100%. 

86.77%. 

76.12%. 

51-65%. 

25.81%. 

0%. 

20 

2-5 

II  .0 

23.0 

70-0 

140 

J95 

30 

4.0 

14.0 

32  .0 

90.0 

165 

230 

40 

5-o 

18.0 

43-o 

115  .0 

196 

277 

50 

6.0 

24.0 

55-o 

144.0 

244 

365 

60 

7-5 

30.0 

70.0 

183.0 

320 

70 

9.0 

41  .0 

93-o 

230.0 

80 

10.5 

56.0 

NOTE.  —  The  figures  in  the  preceding  table  were  read  from  curves 
shown  in  the  abridged  report  of  the  work,  and  are  therefore  only 
approximately  correct.  Determinations  of  the  solubility  in  methyl 
alcohol  solutions  were  also  made  but  not  quoted  in  the  abstract.  The 
"  Synthetic  Method"  (see  Note,  page  9)  was  used. 

100  grams  absolute  ethyl  alcohol  dissolve  4.6  grams  NH4NO3  at 
14°  and  3.8  grams  at  20.5°. 

100  grams  absolute  methyl  alcohol  dissolve  14.6  grams  NH4NO3  at 
14°  and  17.1  grams  at  20.5°. 

(Schiff  and  Monsacchi  —  Z.  physik.  Chem.  21,  277,  '96;  at  2o.s°de  Bruyn  —  Ibid.,  10,  783,  '92.) 


AMMONIUM  MAGNESIUM  NITRATE    2NH4NO3.Mg(NO3)2. 
100  parts  water  dissolve  10  parts  salt  at  12.5°. 

(Foucroy.) 

AMMONIUM  MANGANIC  MOLYBDATE  5(NH4)2MoO4.Mn2(Mo2O7)8. 
i2H2O. 

100  parts  water  dissolve  0.98  Darts  salt  at  17°. 

(Struve  —  J.  pr.  Chem.  61,  460,  '54.) 

AMMONIUM   OXALATE     (NH4)2C2O4. 

100  grams  H2O  dissolve  2.215  grams  (NH4)2C2O4  at  o°  Sp.  Gr.  of 
solution  =  1.0105. 

(Engel  —  Ann.  chim.  phys.  [6]  13,  359,  '88.) 


SOLUBILITY  OP  NEUTRAL  AMMONIUM  .  OXALATE  IN  AQUEOUS    SOLU 
TIONS  OF  ACID  AMMONIUM  OXALATE. 

(Engel.) 

J  Milligram  Mols.  per  10  Grams  per  too  cc. 

cc.  Solution.  Solution. 


(NH4)2C204 

3.54  o-o  2.19  o.o 

2-65  1.45  1.63  0-77 

2-475          2-525  i-52  1-34 

2.38         2.90  1.47  1.54* 

*  Both  salts  present  in  solid  phase 


3i  AMMONIUM    OXALATE 

SOLUBILITY  OP  AMMONIUM  OXALATE  AND  OXALIC  ACID  IN  WATER  AT  25°. 

(Walden  — Am.  Ch.  J.  34,  M9,  '05-) 

Mixtures  of  the  two  substances  were  dissolved  in  warm  water  and 
the  solutions  allowed  to  cool  in  a  thermostadt  held  at  25°. 

Composition  of  Solution. 


Grams  per  100  Gms. 
Solution. 

Mols.  per  100  Mols. 
H20. 

Solid  Phase. 

(NH,) 

2C2O4 

H2C 

(NH4)2C204 

.  H2C204. 

0 

.28 

IO 

2O 

0.045 

2 

.281 

H2C2O4.2H2O  and  (NH4)2C2O4.3H2C2O4.4I 

O 

.46 

7 

24 

0.072 

I 

•570' 

2 

3 

•44 
•65 

2 
2 

•59 
.80 

0.372 
0.566 

0 
0 

•546 

•599 

•       Double  salt,  (NH4)2C2O4.3H2C2O4.4H2O 

4 

5 

•99 
.20 

3 

3 

•55 

0.791 
0.824 

0 
0 

•745  J 
.781 

(NH4)2C2O4.3H2C204.4H2O  and 
(NH4)2C204.H2C204.H20 

5 

•36 

3 

•38 

0.853 

0 

•741 

| 

6 

.27 

3 

.04 

I  -OO 

0 

.671  1 

>        Double  salt,  (NH4)2  .C2O4  .H2C2O4  .H2O 

7 

•03 

2 

.90 

I-I3 

O 

•645  ' 

1 

7 

.08 

2 

.70 

I.I4 

0 

•599 

(NH4)2C204.H2C204.H20  and  (NH4)2C2O4 

6 

.92 

0-775 

(NH4)2C204 

AMMONIUM   HYDROGEN  PHOSPHITE     (NH4H)HPO3. 

100  grams  water  dissolve  171  grams  (NH4H)HPO3  at  o°,  190  grams 
at  14.5°  and  260  grams  at  31°. 

(Amat.  —  Compt.  rend.  105,  809,  '87.' 

AMMONIUM  PERMANGANATE     NH4MnO4. 

100  parts  water  dissolve  approximately  8  parts  of  NH4MnO4  at  15°. 

(Aschoff.) 

AMMONIUM   FLUO   SILICATE   (NH4)2SiF6. 
100  parts  water  dissolve  18.5  parts  (NH4)2SiF,5  at  17.5°,  Sp.  Gr.  1.096. 

(Stolba  — Chem.  Centr.  418,  1877.) 

AMMONIUM  SALICYLATE  C6H4(OH)COONH4. 

100  parts  H2O  dissolve  m.i  parts  C6H4(OH)COONH4  at  25°;  100 
parts  alcohol  dissolve  43.5  parts  at  25°  and  100  parts  at  the  b.  pt. 
(U.  S.  P.) 

AMMONIUM  SULPHATE  (NH4)2SO4. 

SOLUBILITY  IN  WATER. 

(Mulder.) 

^0        Grams  (NH4)2SO4  per  100  Grams.         ft0  Grams  (NH4)2SO4  per  100  Grams. 

Water.  Solution/ 

78.0  43-8 

81.0  44-8 

88.0  46.8 

95-3  48.8 

103.3  5°  8 

107.5  S1-8 
Sp.  Gr.  of  saturated  solution  at  15°  -  1.248;  at  19°  =  1.241. 


t    . 

Water. 

Solution. 

i«    • 

O 

70.6 

41.4 

30 

5 

71.8 

41.8 

40 

10 

73-o 

42.2 

60 

15 

74-2 

42.6 

80 

20 

75-4 

43-o 

100 

25 

76.7 

43-4 

108.9 

AMMONIUM  SULPHATE  32 

SOLUBILITY    OF   MIXTURES    OF   AMMONIUM    SULPHATE    AND    COPPER 

SULPHATE  AT  16°,  AND  OF  AMMONIUM  SULPHATE  AND 

POTASSIUM  SULPHATE  AT  19.1°. 

(Rudorff  — Ber.  6,  482,  '73-) 
(NH^jsSO,  +  CuS04.  (NH4)2S04 


G. per  100  g. Solution.  .  ,     .          G.per  loog.Solution 

Preparation  of  Solution.         ,__--_  Preparation  of  Solution.       __-*__ 


Both  salts  in  excess  8.55  7.12  Both  salts  in  excess  39.3  37.97 

1 5  cc.  sat.  sol.  +  3  gms.  1 5  cc.  sat.  sol.  +  4  g. 

(NH4)2SO4  1.77  18.16  K2SO4  4-94  33-26 

15  cc.  sat.  soL  +  3  gms.  15  cc.  sat.  sol. +  4  g. 

CuSO4.5H2O               15-85  5.65           (NH4)2SO4                 2.05     40.80 


SOLUBILITY  OF  AMMONIUM  SULPHATE  IN  AQUEOUS  ETHYL  ALCOHOL 

SOLUTIONS. 

(Traube  and  Neuberg  —  Z.  physik.  Chem.  i,  510,  '87;  Bodlander —  Ibid.  ^,  318,  '91;  Schreinemaker  — 
Ibid.  23,  657,  '97  ;  de  Bruyn — Ibid.  32,  68,  'oo;  Linebarger  —  Am.  Ch.  J.  14,  380,  '92.) 

Upper  Layer  Results.  Lower  Layer  Results. 

Grams  per  100  Gms.  Solu-  Qms  C2H,OH      Gms-  (NH4)2SO4  per  100  g. 

tion  at  io°-4o°.  per  100  Gms.  Solution  at: 

C2H6OH.     '(NH4)2S04. 
100  0-0 

80          o.i 
70          0.3 

60  1-4 

So  3-2 

45  4-8 

40  6.6 

35  9-2 

30  12.2 

25  14-6 

NOTE.  —  When  ammonium  sulphate  is  added  to  aqueous  solutions 
of  alcohol,  it  is  found  that  for  certain  concentrations  and  temperatures 
the  solutions  separate  into  two  liquid  layers,  the  upper  of  which  con- 
tains the  larger  percentage  of  alcohol. 

Most  of  the  determinations  which  have  been  made  upon  this  system, 
as  contained  in  the  papers  referred  to  above,  are  given  in  terms  of 
grams  of  ammonium  sulphate,  of  alcohol  and  of  water  per  100  grams 
of  these  three  components  taken  together.  Those  results  which  are 
given  in  other  terms  can  be  readily  calculated  to  this  basis,  and  it  is 
therefore  possible  to  make  a  comparison  of  the  several  sets  of  de- 
terminations by  plotting  on  cross-section  paper  and  drawing  curves 
through  the  points.  In  the  present  case  the  grams  of  alcohol  per  100 
grams  of  solution  were  taken  as  ordinates,  and  the  grams  of  ammo- 
nium sulphate  in  the  same  quantity  of  each  solution  taken  as  abscissae. 
It  was  found  that  a  single  curve  could  be  drawn  through  practi- 
cally all  the  points  representing  the  upper  layer  solutions  at  the 
several  temperatures,  but  the  points  for  the  solutions  containing  the 
larger  amounts  of  water  gave  curves  which  diverged  with  increase  of 
temperature.  The  results  given  for  33°  in  the  above  table  are  not 
to  be  accepted  as  correct  until  further  work  has  been  done. 


Solution. 

'6.5°. 

15°. 

33°. 

O 

42.0 

42  .6 

44 

2-5 

39-o 
36.2 

40.2 
37-2 

? 

7-5 

33-2 

34-5 

42 

IO.O 

12.5 
15.0 

30.0 
27.2 
24.6 

31.0 
28.0 
25.2 

35 

17  5 

22  .O 

22  .4 

? 

20.  o 

20.  o 

20.0 

? 

33  AMMONIUM   SULPHATE 

SOLUBILITY  OF  AMMONIUM  SULPHATE  IN  AQUEOUS  PROPYL  ALCOHOL 

SOLUTIONS  AT  20°. 

(Linebarger  —  Am.  Ch.  J.  14,  380,  '92.) 


Gms.  per  100  Gms. 

Gms.  per  100  Gms. 

Solution. 

Solution  . 

CjjHrOH.       (NH4)2S04: 

C3H7OH.       (NH4)2SCv 

70                 0-4 

40             3.2 

60            i.o 

30            4-8 

50                  2.0 

20                  6.7 

AMMONIUM  OADIIITTM  SULPHATE     (NH4)2Cd(SO4)26H2O. 
100  cc.  H2U  dissolve  72.3  grams  (NH4)2Cd(SO4)2  at  25°. 

(Locke  —  Am.  Ch.  J.  27,  459,  'ot.) 

AMMONIUM    CHROMIUM    SULPHATE    (Alum)    (NH4)2Cr2(SO4)4. 

24H2O. 

100  cc.  H2O  dissolve  10.78  grams  anhydrous  or  21.21  grams  hydrated 
salt  at  25°. 

(Locke  —  Am.  Ch.  J.  26,  174,  '01.) 

AMMONIUM  COBALT  SULPHATE     (NH4)2Co(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 


(Tobler  —  Liebig's 

t°. 

O 
10 
2O 
25 
30 

Annalengs,  193,  '55;  v.  Hauer—  J.  pr. 
Ch.  J.  27.  459.  '01.) 

Gms.  (NH4)2Co(SO4)2 
per  TOO  Gms.                             t°. 

Chem.  74.  433.  '58;  at  25°,  Locke—  Am. 

Gms.  (NH4)2Co(SO4)2 
per  100  Gms. 

Water.             Solution. 

6.0            5.7 
9-5            8.7 
13.0          11.5 
14.72         12.8 
17.0          14-5 

40 

50 
60 
70 
80 

Water.         Solution. 
22.  0            l8.O 
27-0            21-3 

33-5        25.1 
40.0        28.6 
49.0      32.9 

NOTE.  —  The  determinations  reported  by  the  above  named  inves- 
tigators were  plotted  on  cross-section  paper  and  although  considerable 
variations  were  noted,  an  average  curve  which  probably  represents 
very  nearly  the  true  conditions  was  drawn  through  them,  and  the  above 
table  made  from  this  curve. 

AMMONIUM  COPPER  SULPHATE     (NH4)2Cu(SO4)2.6H2O. 

100  grams  H2O  dissolve  26.6  grams  salt  at  19°,  Sp.  Gr.  of  sol.  =  1.1336 

(Schiff  —  Liebig's  Ann.  109,  326,  '59.) 

AMMONIUM  IRON  SULPHATE     (Alum)     (NH4)2Fe2(SO4)4.24H2O. 
100  cc.  H2O  dissolve  44.15  gms.  anhydrous  or  124.40  gms.  hydrated 
salt  at  25°.     Sp.  Gr.  of  saturated  solution  at  15°  =  1.203. 

(Locke  —  Am.  Ch.  J.  26,  174,  '01.) 

AMMONIUM  IRON  SULPHATE  (ferrous)     (NH4)2Fe(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 

(Tobler;  at  25°,  Locke  —  Am.  Ch.  J.  27,  459,  '01.) 

fto       G.  (NH4)2Fe(S04)2     to  G.  (NH4)2Fe(SO4)2         t<J  G.  (NH4)2Fe(SO4)2 

per  100  g.  H2O.  per  100  g.  H2O.  per  100  g.  H2O. 

o     12.5     25     2S-o(T)     50       40 
15     20.0     25     35 .i  (L)    70      52 
40     33-o 


AMMONIUM    INDIUM  34 

SULPHATE 

AMMONIUM  INDIUM  SULPHATE     (NH4)2In2(SO4)4.24H2O. 
100  g.  H2O  dissolve  200  gms.  salt  at  16°  and  400  gms.  at  30°. 

(Rossler  — J.  pr.  Chem.  [2]  7,  14.  '73-) 

AMMONIUM    MAGNESIUM   SULPHATE     (NH4)2Mg(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 

(Average  curve,  from  results  of  Mulder,  Tobler,  Locke,  at  25°.) 

G.  (NH4)2Mg(SO4)2  G.  (NH4)2Mg(SO4)2 

4;°^  per  loo  Gms.  t°.  per  100  Gms. 

Water.         Solution.  Water.          Solution. 

o  9.0  8.8  40  27.0  21.3 

10  13.0  11.5  50  32.0  24.4 

20  18.0  15.3  60  37.0  27.0 

25  19.9  16.6  70  42.0  29.6 

30  22.0  l8-0  80  47-0  32.0 

AMMONIUM   MANGANESE  SULPHATE     (NH4)2Mn(SO4)2.6H2O. 
100  cc.  water  dissolve  37.2  gms.  (NH4)2Mn(SO4)2  at  25°. 

(Locke  —  Am.  Ch.  J.  27,  459,  *oi.) 

AMMONIUM  NICKEL  SULPHATE     (NH4)2Ni(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 

(Average  curve  from  Tobler,  Locke,  at  25°.) 

G.  (NH4)2Ni(S04)2  G.  (NH4)2Ni(S04)2 

t°  per  zoo  Gms.  t°.  P61"  I0°  Gms. 


Water.  Solution.  Water.          Solution. 

o  i.o  o-99  4o  12.  o  10.72 

10  4.0  3-85  50  14.5  12.96 

20  6.5  6.10  60  17.0  14-53 

25  7.57  7.04  70  20.0  16.66 

30      9.0        8.45 

AMMONIUM  SODIUM  SULPHATE     NH4NaSO4.2H2O. 

100  gms.  water  dissolve  46.6  gms.  NH4.NaSO4.2H2O  at  15°,  Sp.  Gr. 
Sol.  =  1.1749. 

AMMONIUM  VANADIUM    SULPHATE  (Alum)       (NH4)2V2(SO4)4. 

24H20. 
100  cc.  H2O  dissolve  31.69  gms.  anhydrous  or  78.50  gms.  hydrated 

Salt  at  25°.  (Locke.) 

AMMONIUM  ZINC  SULPHATE     (NH4)2Zn(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 

(Average  curve,  see  Note,  p.  33,  Tobler,  Locke,  at  25°.) 

G.  (NH4)2Zn(S04)2  G.  (NH4)2Zn(SO4)2 

t°.  per  IPO  Gms.  40  per 


Solution.  Water.  Solution.  Water. 

o    6.54  7.0  40  16.66  20 

10      8.67  9.5  50  20-0  25 

20     1  1.  1  1  12-5  60  23.1  30 

25    12.36  14.1  70  25.9  35 

30    13-79  16.0  80  29.6  42 


35     AMMONIUM   PERSULPHATE 
AMMONIUM   PERSULPHATE     (NH4)2SaO8. 

100  parts  H2O  dissolve  58.2  parts  (NH4)2S2O8  at  o°. 

(Marshall  —  J.  Chem.  Soc.  59,  771,  '91.) 

AMMONIUM  SODIUM  HYDROGEN  SULPHITE    (NH4)Na2H(SO3)2 
4H20. 

100  gms.  H2O  dissolve  42.3  gms.  salt  at  12.4°  and  48.5°  gms.  at  15°. 

(Schwincker  —  Ber.  22,  1732,  '89.) 

AMMONIUM  SULPHOCYANIDE     NH4SCN. 

100  parts  water  dissolve  128.1  parts  NH4SCN  at  o°  and  162.2  parts 
at  20°. 

(Clowes  — Z.  Ch.  190,  1866.) 

AMYL  ACETATE  BUTYRATE,   FORMATE,  etc. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ALCOHOL  AT  20°. 

.(Bancroft —  Phys.  Rev.  3,  131,  196,  205,  '95~'96;  Traube.  —  Ber.  17,  2304,  '84.) 

v  .  ,  cc.  Ester  per        Sp.  Gr.  F  .  cc.  Ester  per  Sp.  Gr. 

ioocc.H20.        of  Ester.  100  cc.  H2O.  of  Ester. 

Amyl  acetate       0.2  0.88     Amyl  propionate    o.i  0.88 

Iso  amyl  acetate  0.2(1.2?)      ...     Iso  amyl  formate    o .  3  (gms.  at  22°) 
Amyl  but y rate    o . 06  0.85 

Solubility  of  Iso  Amyl  Acetate  Solubility  of  Amyl  Acetate  and  Amyl 
in  Aq.  Alcohol  Mixtures.  Formate  in  Aq.  Alcohol  Mixtures. 


cc.  H2O  added  to  cause  separation 
of  second  phase  in  mixtures  of  the 


Per  5  cc.  C2H5OH. 

,_  TT  0          cc.LsoAmyi 
acetate. 

7  0.41 

6  0.7 

5  1-31 

3.61        3.0 

3.01        4.0 

2 . 60  5-O 


cc.  C2H5OH 
in  Mixture. 

given  amounts  ot  ale 
portions 

:ohol  and 
of: 

Amyl 

Amyl 

Formate. 

Acetate. 

3 

1.  80 

I.76 

9 

8-77 

9-03 

15 

17.01 

I7-52 

21 

27.06 

26.99 

27 

38-3I 

37-23 

33 

5°-7l 

48.41 

39 

65  .21 

45 

85.10 

48 

94-20 

ANETHOL  (p  Propylanisol)  CH3CHCH[4]C6H4OCH3. 
SOLUBILITY  IN  AQ.  ALCOHOL  AT  20°. 

(Schimmel  and  Co.  Reports,  Oct  1895,  p.  6-) 

Vol.  per  cent  alcohol  =  20  25  30         40  5° 

Gm.  Anethol  per  liter  aq.  alcohol=o.i2       0.20        0.32     0.86        2.30 


ANILINE 


36 


ANILINE     C6H5(NH2). 

SOLUBILITY  IN  WATER  AT  22°. 

(Herz  —  Her.  3  1,  2671,  '98;  see  also  Vaubel  —  J.  pr.  Chem.  [2)  52,  72,  '95:  Aignan  and  Dugas  — 
Compt.  rend.  129,  643,  99.  ) 

ioo  cc.  H2O  dissolve  3.481  cc.  C6H5(NH2)  —  Vol.  of  Sol.  =  103.48, 
Sp.  Gr.  =  0.9986. 

ioo  cc.  C6H5(NH2)  dissolve  5.22  cc.  H2O  —  Vol.  of  Sol.  =  104.96, 
Sp.  Gr.  =  1.0175. 

SOLUBILITY  OF  ANILINE  IN  WATER  AT  DIFFERENT  TEMPERATURES. 

(Alexejew  —  Ann.  Physik.  Chem.  28,  305,  '86;  calc.  by  Rothmund  —  Z.  physic.  Chem.  26,  475,  '98.) 
Determinations  by  "  Synthetic  Method  "  see  Note,  p.  9.    Figures  read  from  curve. 

0  Gms.  CfiHfiNH2j3er  ioo  Grams. 

Aq.  Layer.     Aniline  Layer. 
140  13.0 

150  18.0 

160  27.5 

l65  36-° 

167.  5  (crit.  temp.)  48.6 


Gms.  Cfi  Hs(NH2)  per  ioo  Grams. 


I  . 

Aq.  Layer. 

Aniline  Layer. 

20 

3-2 

95-5 

40 

3-5 

95-o 

60 

3-8 

94-7 

80 

4-5 

93-5 

ioo 

6.0 

92  o 

120 

8-5 

88.s 

83.5 

79.0 
71.0 
63-° 


SOLUBILITY  OF  ANILINE  IN  AQUEOUS  SALT  SOLUTIONS  AT  18°. 

(Euler  —  Z.  physik.  Chem.  49,  307,  '04.) 

Gms.  Salt     Gms-  C6H5(NH2) 
per  liter,     per  ioo  g.  solvent. 

o  3.61  N 

37.3          3.15  N 

74-6          2.68  N 


A      q  i«ti 

H2O  alone 
N      KC1 
N     KC1 


Aq. 
Solution. 


Gms.  Salt    Gms.C6H6(NH2) 
per  liter,    per  ioo  g.  solvent. 

NaOH  40.06  1.90 
Lid  42.48  2.80 
CuCl2  67.25  3.00 


Per  cent  C6H5NH2.HC1      Gms.  C6H6NH2 
in  Solvent.  per  ioo  g.  Sol  vent. 


N    Nad        58.5  2.55 

SOLUBILITY  OF  ANILINE  IN  AQUEOUS  ANILINE  HYDROCHLORIDE 
SOLUTIONS  AT   18°. 

(Lidow  —  J.  russ.  phys.  chem.  Ges.  15,  420,  '83;  Ber.  16,  2297,  '83.) 

Per  cent  C6H5NH2HC1    Gms.  C6N6NH2 
insolvent  per  ioo  g.  Sol  vent. 

5  3-8  30  39-2 

12  5-3  35  5o-4 

25  18.3 

DISTRIBUTION  OF  ANILINE  BETWEEN: 

(Vaubel  —  J.  pr.  Chem,  [2]  67,  477,  '03.) 

Water  and  Ether.  Water  and  Carbon  Tetrachloride. 

Composition  of  Solutions.          Gms.  CeHsNE^in:         Composition  of  Solutions.     Gms.CcHsNFb  in: 

'  Aq.         CC14  * 

Layer.     Layer, 


G.C6H5NH2          s, 
Used 

1.2478     50  cc.  H2O 

+  2occ.  Ether     0.1671 
1.2478     50  cc.  H2O 


Aq  EtheT     G.  C8H6NHa 

Layer.          Layer.  Used. 

50  cc.  H2O 
1.0807     °-3478      +2occ.CCl4     0.3358  0.012 

50  cc.  H2O 

+  5occ.  Ether     0.0835     I-l643     1.2478     +5occ.CCl4     0.2767   1.971 
1.2478     50  cc.  H.,0  50  cc.  H2O 

-f  ioo  cc.  Ether  0.0594     1.1884     1.2478     4-ioocc.  CC14  0.1845   1-°63 

SOLUBILITY  OF  ANILINE  IN  SULPHUR. 

(Alexejew  —  Ann.  Physik.  Chem.  28,  305,  '86.) 


to 

ioo 
no 
120 


Gms.C6H5NH2  per  ioo  g. 
S.  Layer.     Anilin  Layer. 

4  75 

6  70 

TO  64 


Gms.  C6H5NH2  per  ipog. 
S.  Layer.      Anilin  Layer. 

*3o  15  58 

135  17.5  47 

138  (crit.  temp.)          23 


37 


ANILINE 


DISTRIBUTION  OF  ANILINE  BETWEEN  WATER  AND  TOLUENE  AND 
BETWEEN  AQUEOUS  SALT  SOLUTIONS  AND  TOLUENE  AT  25° 

(Ricckl  —  Z.  physik.  Chem.  56,  243,  '06.) 

NOTE.  —  Mixtures  of  Aniline  and  Toluene  were  shaken  with  water  or 
with  aqueous  salt  solutions,  and  after  separation  of  the  two  layers  the 
Sp.  Gr.  of  the  A  :  T  mixture  (layer)  was  determined  and  also  the  amount  of 
Aniline  in  each  layer. 


Solution  Shaken  with 
A  :  T  Mixture. 

Vol.  per  cent     ! 
Aniline  :  Toluene 
in  Mixtures  Used. 

Sp.  Gr.  of  A  :  T 
Mixture  after 
Separation. 

'    Gms.  QHsN 

H2  in  100  cc.  of: 

A  :  T  Layer. 

Aq.  Layer. 

H20 

50:50 

0-9257 

41-5 

2.14 

a 

25:75 

0.8928 

20-7 

11 

12.5:87.5 

0.8737 

8.62 

0.86 

" 

5-5:94-5 

0.8661 

3-87 

o-45 

(C 

2-5:97-5 

0.8627 

1.68 

O-2I 

XT         K2S°4 

o.iN    —  -  —  - 

2 

50:50 

0.9297 

44-o 

2.09 

" 

25:75 

0.8901 

19.03 

I.38 

it 

12.5:87.5 

0.8739 

8-77 

0.81 

it 

5-5:94-5 

0.8663 

3-94 

0.42 

n 

0.8629 

1.81 

O.2I 

o.iN    KBO2 

50:50 

0-9257 

41  .61 

2  .11 

u 

25:75 

0.8870 

17.08 

i-34 

« 

12.5:87.5 

0.8748 

9-34 

0.92 

" 

5-5:94-5 

0.8661 

3-85 

o-44 

a 

2-5:97-5 

0.8627 

1.72 

O.2I 

XT           -DclfO-H.).) 

o.oio94N     —  -  a 

2 

50:50 

o-9334 

46.52 

2  .IO 

it 

25:75 

0.8929 

20.78 

I  .46 

11 

12.5:87.5 

0.8749 

9.41 

0.88 

it 

5-5:94-5 

0.8663 

3  -96 

o-43 

tl 

2-5:97-5 

0.8628 

1.72 

O-2O 

XT    Sr(OH)2 
o.io4N 

50:50 

0-9333 

46-45 

2.13 

2 

It 

25:75 

0.8929 

20.78 

1  .46 

~     Sr(OH), 
o  .  IO44-IN      —  *  — 

12.5:87.5 

0.8750 

9.46 

0.88 

2 

it 

5-5:94-5 

0.8662 

3.96 

o-43 

s      AT           oT(  VyXlJo 

O  •  1  003  IN        

2.5:97-5 

0.8628 

1.75 

0-2O 

2 

~,TVT     Ca(OH)2 

50:50 

0-9333 

46.18 

2  .20 

2 

n 

25:75 

0.8925 

20.59 

1.51 

a 

12-5:87.5 

0.8749 

9-43 

0.91 

" 

5-5:94-5 

0.8662 

3-89 

0-44 

n 

2.5:97-5 

0.8627 

1.70 

O-2I 

ioo  cc.  aqueous  solution  contain  3.607  gms.  Aniline  at  25°. 


ANILINE 


SOLUBILITY  OF  ANILINE,  PHENOL  MIXTURES  IN  WATER. 

(Schrcinemaker  — Z.  physik.  Chem.  29,  584;  30,  460,  'gg.) 


Mixture  used  =  25.4  Mols.  Aniline 

-f-  74  6  Mols.  Phenol 
Gms.  of  Mixture  per  100  Gms. 


Mixture  used  =  50  Mols.  Aniline 
+  50  Mols.  Phenol 


Aq.  Layer.     A. 

+  P.  Layer 

40 

5 

.0 

86.0 

40 

60 

5 

•5 

82.0 

80 

80 

8 

•  o 

77.0 

IOO 

IOO 

12 

•5 

67.0 

120 

no 

19 

.0 

56.5 

I30 

104 

(crit.  temp.) 

33 

135 

a  =  50 

Mols. 

Gms.  of  Mixture  per  100  Gms. 

Aq.  Layer.    A.  +  P.  Layer. 
4-0 

5-5 
8.0 


85-5 
82.0 


19.0 
23-5 


73-5 
66.0 
58.0 


140  (crit.  temp.)        35       ... 
Determinations  in  above  table  by  "Synthetic  Method,"  see  NOTE,  p.  9. 
Schreinemaker   gives   results   for   several  other   mixtures  of   Aniline  and 
Phenol  which  yield  curves  entirely  similar  to  those  for  the  two  mixtures 
here  shown. 

NitrANILINES      C6H4NH2NO2.     o,  m,  and  p. 
SOLUBILITY  IN  WATER. 

(Carnelly  and  Thomson  —  J.  Chem.  Soc.  53,  768,  '88;  Vaubel  —  J.  pr.  Chem.  [2]  52,  73,  'gs;  above  ao°, 
Lowenherz —  Z.  physik.  Chem.  25,  407,  'g8.) 

Grams  NItraniline  per  Liter  of  Solution. 

t°.  , *--  —^ 

Ortho  Nitranilinc.     Meta  Nitraniline.     Para  Nitraniline. 
20  I.I4-I.67  0.77-0.80 

24.2  1.25   (25°)          1.205 

27.3  1.422 

SOLUBILITY  OF  ORTHO  AND  OF  META  NITRANILINE  IN  HYDROCHLORIC 

ACID. 

(Lowenherz.) 


Ortho  Nitraniline  at  25°. 

G.  Mols.  per  Liter.         Grams  per  Liter. 


Meta  Nitraniline. 

G.  Mols.  per  Liter.          Grams  per  Liter. 


'HCl 

CGH5NH2. 

HCl      CeHsNHa. 

'HCl 

C6H5NH2. 

HCl        C6H5NH2. 

*02(o) 

N( 

^2(0) 

NO2(w) 

NO2(7w) 

o.o 

0 

.0091 

o.o 

I 

•25 

(25° 

) 

0-0 

o  .0091 

o.o 

1.20 

0.63 

0 

.0143 

22-97 

I 

•97 

(26. 

5°) 

0.0125 

0-0183 

0.46 

2-53 

0.95 

0 

.0174 

34.63 

2 

.40 

(23- 

3°) 

0.0247 

0.0274 

0.90 

3.85 

i  .26 

0 

.0215 

45-94 

2 

•97 

SOLUBILITY  OF  META  AND  OF  PARA  NITRANILINE  IN  ORGANIC 
SOLVENTS  AT  20°. 

(Carnelly  and  Thomson.) 


Solvent. 

Methyl  Alcohol 
Ethyl  Alcohol 
Propyl  Alcohol 
Iso  Butyl  Alcohol 
Iso  Amyl  Alcohol 
Ethyl  Ether 


Gms.  per  Liter. 
Para. 

95-9 

58-4 

43-5 
19.1 
62  .9 
61  .o 


Meta. 

no.  6 

70-5 

56-5 
26.4 
85.1 
78.9 


Solvent. 

Benzene 

Toluene 

Cumene 

Chloroform 

Carbon  Tetra  Chloride 

Carbon  Bisulphide 


Gms.  per  Liter. 


Meta. 

24-5 
I7.I 

"•5 

30.1 

2  .1 

3-3 


Para. 
19.8 

I3-I 

9-0 
23.1 

i-7 

2.6 


ANISIC  ACID  (p-Methoxybenzoic  acid)  CH3O.CGH4.COOH.  See  also  p.  61. 
loo  cc.  sat.  aq.  solution  contain  0.2263  gm-  Anisic  acid  at  25°. 

(Paul  —  Z.  physik.  Chem.  14,  in,  '94.) 


39 
ANTHRACENE     C14H10. 

SOLUBILITY  IN  LIQUID  SULPHUR  DIOXIDE  IN 


ANTHRACENE 


THE  CRITICAL  REGION. 

(Centnerswer  and  Teletow  —  Z.  Electrochem.  g,  799,  '03.) 


Weighed  amounts  of  anthracene  and  liquid 
tubes  which  were  then  sealed,  rotated  at 
temperature  and  the  point  at  which  the  solid 


SO2  were  placed  in  glass 
a  gradually  increasing 
disappeared,  observed. 


Grns. 
per  100  g 
Solution. 


40.1 
45-8 
47-9 


2  .II 
2.48 
2  .65 


65.0 

78.2 

88.0 


Cms.  Cu  H10 
per  loo  g. 
Solution. 

4-0 

5-66 

7.14 


98.0 

99-1 

106.5 


Cms.  Cu  Hj 
per  loo  g. 
Solution. 

9  36 

9  95 
12.78 


SOLUBILITY  OF  ANTHRACENE  IN  ABSOLUTE  ETHYL  AND  METHYL 

ALCOHOLS. 

(v.  Becchi;  at  19.5°,  de  Bruyn  —  Z.  physik.  Chem.  10,  784,  '92.) 

Grams  Ci4Hio  per  100  Grams  Alcohol  at; 


1 6° 


In  Ethyl  Alcohol 
In  Methyl  Alcohol 


0.076 


19-5  • 
1.90 
i. 80 


b.pt. 
0.83 


SOLUBILITY  OF  ANTHRACENE  IN  BENZENE. 

(Findlay  —  J.  Chem.  Soc.  81,  1221,  '02.) 


t°. 

Gms.  CMH10 
per  100  Gms. 

Mols.  CuH,o 
per  loo  Mols. 

C6H6. 

CeH6. 

5 

0-979 

0.429 

10 

1.118 

0.491 

15 

1  .296 

0-567 

20 

1-532 

0.673 

25 

1.830 

0.803 

26.5 

I-951 

0.856 

30 

2-175 

o-954 

100  parts   of  toluene  dissolv 
12.94  parts  at  100°  (v.  Becchi). 


t°. 

Gms.  C14H10 
per  100  Gms. 

Mols.  C14H19 
per  100  Mols. 

C6H6. 

CeHg. 

38-4 

2-773 

I.2I3 

40.0 

2-987 

I.3I2 

44.6 

3-368 

1-473 

50 

3.928 

1.727 

60 

4.941 

2  .164 

70 

6.041 

2.649 

80 

7-175 

3-M3 

irts  anthracene  at 

16.5°  and 

SOLUBILITY  OF  ANTHRACENE   IN  ALCOHOLIC  PICRIC  ACID  SOLUTIONS 

AT    25°. 
(Behrend  —  Z.  physik.  Chem.  15,  187,  '94.) 


Grams  per  100  Grams 
Solution. 


Picric 
Acid. 

O 

I.OI7 
2.071 
2.673 

3-233 


Solid  Phase. 


Anthracene. 

0.176    Anthracene 

0.190 

0.206 

0.215 

0.228 


3.469     0.236 


Grams  per  100  Gms. 
Solution . 


Anthracene  and 
Anthracene  Picrate 


Picric 
Acid. 

3-999 

5.087 

5-843 
6.727 

7-511 
7-452 


Anthracene . 

O.2O2 
0-lSo 

o .  162 

O.I5I 
0.149 


Solid  Phase. 


Anthracene  Picrate 


Anthracene   Picrate 

-f-  Picric  Acid 
Picric  Acid 


Gms.  Ci4H8O2 

Gms.  CUH8 

t°. 

per  100  g. 
Solution. 

t°. 

per  100  g. 
Solution. 

92.1 

2.81 

IlS-5 

5.60 

IOI-4 

3-67 

141  .6 

7-53 

106.3 

4-23 

160.0 

9.60 

108.7 

4-40 

179.0 

12.70 

183-7 

18.30 

ANTHRAQUINONE  40 

ANTHRAQUINONE  (C6H4)2(CO)2. 

SOLUBILITY  IN  LIQUID  SULPHUR  DIOXIDE  IN  THE  CRITICAL  REGION. 

(Centnerswer  and  Teletow  —  Z.  Electrochem.  9,  799,  '08.)     (See  Anthracene,  page  39). 

Gms.  QuHsOjs 
t°.  per  100  g. 

Solution. 

39.6  0.64 

51.5  0.88 

67.9  1.73 

82.4  2.24 

100  parts  of  absolute  ethyl  alcohol  dissolve  0.05  part  anthroquinone 
at  18°  and  2.249  parts  at  b.  pt.  (v.  Becchi). 


SOLUBILITY  OF  ANTHRAQUINONE  IN  ETHER. 

(Smits  — Z.  Electrochem.  9,  663,  '03.) 

Weighed  amounts  of  ether  and  anthraquinone  were  placed  in  glass 
tubes  which  were  then  sealed.  The  temperature  noted  at  which  the 
anthraquinone  disappeared  and  also  at  which  the  liquid  phase  disap- 
peared (critical  temp.).  The  two  curves  cross  at  195°  and  again  at 
241°.  Between  these  two  temperatures  the  critical  curve  lies  below 
the  solubility  curve,  hence  for  this  range  of  temperature  no  solubility 
curve  is  shown.  The  following  figures  were  read  from  the  curves,  and 
are  therefore  only  approximately  correct. 


Gms.  Ci4H8O2  Gms.  CuHsO2                         Gms. 

t°.             per  100  g.                           t°.  per  100  g.  t  °»           per  100  g. 

Solution.  Solution.                                   Solution. 

130     3         241  30  260    80 

150     4          245  40  270    90 

170     4-5        247  So  275    100 

195     5 .o        250  60 

100  parts  of  toluene  dissolve  0.19  part  anthraquinone  at  15°  and 
5.56  parts  at  100°  (v.  Becchi). 


ANTIMONY  TRICHLORIDE     SbCl3. 

SOLUBILITY  IN  WATER.     SOLID  PHASE  SbCl3. 

(Meerburg  —  Z.  anorg.  Chem.  33,  299,  1903.) 

Mols.  SbCl3                 Gms.  SbCla                                          Mols.  SbCl3  Gms.  SbCl3 

t°.         per  100                         per  100                            t°.                   per  100  per  100 

Mols.  H2O.                    g.  H2O.                                              Mols.  H2O.  g.  H2O. 

o   47-9       601.6        35      91.6  1152.0 

15    64.9       815.8        40     108.8  1368.0 

(72.4       910.1        50     152.5  1917.0 

(74-i                  93*-5                   60            360.4  453I-o 

25         78.6                  988.1                    72                 oo  oo 
30        84.9                1068. o 


4i         ANTIMONY   TRICHLORIDE 

SOLUBILITY  OF  ANTIMONY  TRICHLORIDE  IN  AQUEOUS  HYDROCHLORIC 
ACID.    SOLID  PHASE  SbCl3.     TEMP.  20°. 

(Meerburg.) 


Mols.  per 
100  Mob.  H2O. 

Gms.  per 
100  g.  H2O. 

Mols.  per 
100  Mols.  H2O. 

Gms.  per 
100  g.  H2O. 

'HC1.        SbCla.' 

o        72.4 

2-4      71.2 

6.1     69.9 
8.3     68.2 

HC1.          SbCla. 

o.o      910.1 

4-86      895.4 
12-34      879.0 

16.80    857.6 

HC1.            SbCla". 
9-1            68.9 

11.7        68.1 

28.7      62.8 

HC1.         SbCl* 
18.41      866.4 
23.68      856.3 
58.08      789.8 

100  grains  absolute  acetone  dissolve  537.6  grams  SbCl3  at  18°. 

(Naumann  —  Ber.  37,  4332,  '04.) 

ANTIMONY    TRI   IODIDE     SbI3. 

SOLUBILITY  IN  METHYLENE  IODIDE  AT  12°. 

(Retgers  — Z.  anorg.  Ch.  3,  344,  '93.) 

ioo  parts  CH2I2  dissolve  1 1.3  parts  SbI3.     Sp.  Gr.  of  solution  =  3.453. 

ANTIMONY    POTASSIUM    TARTRATE     K(SbO)C4H4O6.iH2O. 
ioo  grams  glycerine  dissolve  5.5  grams  of  the  tartrate  at  15.5°. 

ARGON,   A. 

SOLUBILITY  IN  WATER. 

(Estreicher  — Z.  physik.  Chem.  31,  184,  '99.) 


fto          Cor.  Bar. 

Vol.            Vol.  Absorbed 

Absorption  Coefficients.* 

Solubility. 

Pressure. 

H2O. 

Argon. 

a. 

/. 

q. 

0 

. 

. 

. 

0-0578 

0 

.0102 

I 

764 

•9 

77- 

40 

4 

•34 

O 

.0561 

0-0561 

0 

.0099 

5 

765 

.0 

77- 

39 

3 

.92 

O 

.0507 

o  .  0508 

O 

.OO9O 

10 

765 

•3 

77- 

3 

•49 

0 

.0450 

0-0453 

O 

.0079 

15 

762 

•4 

77- 

46 

3 

•13 

o  .  0404 

O.O4IO 

0 

.0072 

20 

757 

.6 

77- 

53 

2 

.86 

o 

.0369 

0.0379 

O.OO66 

25 

766 

•7 

77- 

62 

2 

.64 

0 

•0339 

0.0347 

O 

.0060 

760 

.6 

77- 

73 

2 

•43 

o 

.0312 

0.0326 

O 

.0056 

35 

757 

.1 

77.86 

2 

.24 

o 

.0288 

0.0305 

0 

.0052 

40 

758 

•3 

77- 

99 

2 

.07 

o 

.0265 

O.O286 

o 

.0048 

45 

756 

•4 

78. 

15 

I 

.92 

0 

.0246 

0.0273 

o 

.0045 

50 

747 

.6 

78. 

31 

I 

•73 

o 

.0221 

0.0257 

o 

.OO4I 

a  =  under  barometric  pressure  minus  tension  of  H2O  vapor. 

/  =  under  760  mm.  pressure. 

q  =  grams  argon  per  ioo  g.H2O  when  total  pressure  is  equal  to  760  mm. 

*  See  Acetylene,  page  8. 

ARSENIC    PENTOXIDE     As2O5. 

ioo  parts  H2O  dissolve  244.8  parts  As2O4  =  302.3  parts  H3AsO4  at 
1 2.5°.  Sp.  Gr.  of  solution  =  2.18  at  15°. 

(Vogel.) 
ARSENIC    IODIDE     AsI3. 

SOLUBILITY  IN  METHYLENE  IODIDE  AT  12°. 

(Retgers  —  Z.  anorg.  Chem.  3,  344,  1893.) 

ioo  grams  CH2I2  dissolve  17.4  gms.  AsI3.     Sp.  Gr.  of  solution  •»  3.449. 


ARSENIC    TRIOXIDE 


42 


ARSENIC    TRIOXIDE 


As2O3. 
SOLUBILITY  OF  THE: 


Crystallized  Modification. 
In  Water. 


Gms.  As2O3 

t°. 

per  100  cc. 

Sat.  Solution. 

2 

I  .201 

IS 

I-657 

25 

2.038 

39-8 

2.930 

b.  pt. 

6.+ 

(Bruner  and  St.  Tolloczko  —  Z.  anorg.  Chem.  37,  456, 
'03;  Chodounsky  —  Listy.  Chem.  13,  114,   '88.) 


Amorphous  Modification. 
In  Water. 

A.O  Gms.  As2O3  per 

100  cc.H2O. 

ord.  temp.          3  . 7 
b.  pt.  11.86 

In  Alcohol,  Ether  and  CS2. 

G.  As2O3  per  100  g.  Solvent. 

Alcohol  o .  446 

Ether  0.454 

CS9  o.ooi 

(Winkler  —  J.  pr.  Chem.  [2]  31,  347,  '85-) 


ASPARAGINE     C4H8N2O3.H2O. 

SOLUBILITY  /S-/-ASPARAGINE  C4H8N2O3.H2O  AND  OF  /S-/-ASPARAGINIC 
ACID  C4H7NO4  IN  WATER. 

Determined  by  "  Synthetic  Method,"  see  Note,  page  9. 

(Bresler  —  Z.  physik.  Chem.  47,  613,  '04.) 


/3-J-Asparagine. 


/3-/-Asparaginic  Acid. 


Gms. 
t°.   C4H8N203.H2O     t°. 
per  100  g. 

Gms. 
C4H8N203.H20 
per  100  g. 

tc 

Gms. 
C4H7NO4 
per  100  g. 

t  °. 

Gms. 
C4H7N04 

per  100  g. 

H2O. 

H20. 

H20. 

H20. 

0-7 

0 

•9546 

55 

•5 

10.650 

o 

2 

o. 

2674 

51.0 

1.2746 

7-9 

I 

.4260 

7i 

•7 

19.838 

9 

•5 

0 

.4042 

63-5 

1.8147 

I7-S 

2 

.1400 

87 

.0 

36-564 

16 

•4 

0 

•5T76 

70.0 

2-3500 

28.0 

3 

.1710 

98 

.0 

52-475 

3i 

•5 

0 

75*4 

8o.s 

3  .2106 

41.4 

5 

.6500 

40 

.0 

0 

.9258 

97-4 

5-3746 

ATROPINE     C17H23NO3. 

SOLUBILITY   OF   ATROPINE   C17H23NO3   AND   OF   ATROPINE   SULPHATE 
(C17H23NO3)2.SO2(OH)2  IN  WATER  AND  OTHER  SOLVENTS. 

(U.  S.  P.  ;  Miiller  —  Apoth.-Ztg.  18,  244,  '03.) 

Grams  Atro- 
Grams  Atropine  per  100  Grams.  pine  Sulphate 

Solvent.  t°.  , ' N  per  100  Grams 

Solution.  Solvent.    (U.  S.  P.)  Solvent. 

(U.  S.  P.) 


Water  25 

Water  80 

Alcohol  25 

Alcohol  60 

Ether  25 

Chloroform  25 

Benzene  20 
Carbon  Tetrachloride     20 

Ethyl  Acetate  20 

Petroleum  Ether  20 

Glycerine  15 


I  .782   (2O0)  O.222 


68.44 
III  .II 

6. 02 
64.10 


*  Schnidelmeiser 


2.21   (20°) 
68.03(20°) 

3-99 
0.661 
3.88 
0.83 

3.0 

—  Chem.  Ztg.  25,  129,  '01. 


1. 136*  (I7°) 


263.1 

454-5 

27.0 

52.6 
0.047 
0.161 


33-o 


43  AZELAIC    AOID 

AZELAIO    ACID  C7H14(COOH)2. 

SOLUBILITY  IN  WATER. 

(Lamouroux  —  Compt.  rend.  128,  998,  '99.) 

t°=  o  15  20  35  50  65 

Gms.  C7H14(C09H)2 
per  100  cc.  solution  =    o.io        0.15  0.24         0.45         0.82          2.20 

AZOPHENETOL  (/>)    C6H5N2.C6H4.OC2H5. 

SOLUBILITY  IN  100  PER  CENT  ACETIC  ACID. 

(Dreyer  and  Rotarski  —  Chem.  Centr.  76,  II,  1016,  '05.) 

t°=  89.2  91  93  95.6  97.2  99.6 

Mols.  per  liter.         0-153     0.176         0.185         0.209         0.232         0.252 

A  knick  at  94.7°  corresponds  to  the  transition  temperature  of  the 
a  modification  into  the  /3  modification. 


BARIUM    ACETATE  Ba(CH3COO)2. 

SOLUBILITY  IN  WATER. 

(Walker  and  Fyffe  —  J.  Ch.  Soc.  83,  179.  '03;  Krasnicki  —  Monatsh.  Chem.  8,  597,  '87.) 

Gms.  Ba(CH3COO)2  Gms.  Ba(CH3COO)2 

t°.           per  IPO  Gms.                     Solid  Phase.  t°.            per  TOO  Gms.          Solid  Phase. 

Water.   Solution.  Water.   Solution. 

0.3     58.8    37.0    Ba(C2H302)2.3H20  40.5     79.0    44.1  Ba(C2H3O2)2 

7-9     61  6     38.1  41.5     78.7     44.0 

17.5  69.2     40.9  44.5     77.9     43.8 

21.6  72.8     42.1  51.8     76.5     43.4 

24.1  78.1     43.9                    "  63.0     74.6     42.7 

26.2  76.4    43-3     Ba(C2Hp2)2.H20  73.0     73.5     42.4 
30.6     75.1     42.9  84.0     74.0    42.5 
35-o     75-8     43-i  99-2     74-8     42-8 
39-6     77-9     43-8 


Transition  temperatures  24.7°  and  41' 


BARIUM    ARSENATE     Ba3(AsO4)2. 

100  gms.  H2O  dissolve  0.055  £m-  Ba3(AsO4)2;  100  gms.  5%  NH4C1 
dissolve  0.195  gm->  and  IO°  gms.  10%  NH4OH  dissolve  0.003  gm- 
Ba3(AsO4)2 

(Field  — J.  Ch.  Soc.  u    6,  1859-) 


BARIUM    BROMATE  44 

BARIUM    BROMATE     BaBrO3.H2O. 

SOLUBILITY  IN  WATER. 

(Trantz  and  Anschiitz  —  Z.  physik.  Chem.  56,  238,  '06;  Rammelsberg  —  Pogg.  Ann.  52,  81,  '41.) 

Gms.  Ba(BrO3)2  Cms.  Ba(BrO3)2  Gms.  Ba(BrO3)j 

t°  per  100  Gms.  t°.  per  100  Gms.  t°.  per  100  Gms. 

Solution.  Solution.  Solution. 

—  0.034  0.28  30  0-95  70  2.922 

o  0.286  40  1.31  80  3.521 

-f-io  0-439  5°  I-72  9°  4-26 

20  0.652  60  2.271  98.7  5-256 

25  0.788  99.65  5.39 

BARIUM    BROMIDE     BaBr2.2H2O. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg.  Ann.  99,  47,  '56;  Etard  —  Ann.  chim.  phys.[7]2,  540,  '94.) 

Gms.  BaBrg  per  I0°  Grams.  Gms.  BaBrg  per  TOO  Grams. 

t°.  'Water.  Solution.  t°.  '  Water.  Solution. 

(Kremers.)     (Kremers.)     (Etard.)  (Kremers.)     (Kremers.)      (Etard.) 

—  20  45-6          4o  114        53-2        5*-5 

o          98        49.5        47-5          5o            n8  54-1  52-5 

10        101        50.2        48.5          60            123  55.1  53.5 

20        104        51.0        49.5          70            128  56.1  54.5 

25        106        51.4        50.0          80            135  57.4  55-5 

30        109        52.1        50-6        100            149  60.0  57-8 

140  59.4 
Sp.  Gr.  of  saturated  solution  at  19.5°  =  1.710. 

The  results  of  Kremers  and  Etard  are  both  given,  since  it  is  uncer- 
tain which  is  the  more  correct. 

SOLUBILITY  OF  MIXTURES  OF  BARIUM  BROMIDE  AND  BARIUM  IODIDE 
IN  WATER  AT  DIFFERENT  TEMPERATURES. 

(Etard.) 
0  Grams  per  100  Gms.  Solution.  Grams  per  100  Gms.  Solution. 

BaBr2. BaI2.  BaBr2. *       Bal^. 

— 16  4.8        58.4  170  ii. o        67.4 

-f6o  5.5        66.0  210  14.9        67.7 

135  9.2        67 .2  Both  sahs  present  in  solid  phase. 

SOLUBILITY  OF  BARIUM  BROMIDE  IN  METHYL  AND  ETHYL  ALCOHOLS. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  783,    92  ;   Richards  —  Z.  anorg.  Chem.  3,  455,  '93  ;  Rohland  —  Ibid. 

15  412,  '97.) 

Parts  BaBr2  per  100  Parts  BaBr2.2H2O  per  100 

t  o  parts  Aq.  C2H6OH  of:  parts  of  Aq.  CH3OH  of: 

100%.         97%-  87%.  100%.  93-5%.  50%. 

15.0       ..  0.48    (BaBr2.2H2O)  ..  45.9  27.3  4-O 

22.5      3  6  56.1 

BARIUM    BUTYRATE     Ba(C4H7O2)2.2H2O. 
SOLUBILITY  IN  WATER. 

(Deszathy  —  Monatsh.  Chem.  14,  249,  '93.) 

Gms.  Ba(C4H7O2)2  per  100  Gms.  Gms.  Ba(C4H7O2)2  per  TOO  Gms. 

Water.  Solution.  Water.  Solution. 

o  37.42  27.24  50  36.44  26.77 

10  36-65  26.82  60  37-68  27.36 

20  36.12  26.55  70  39-58  28.36 

30  35-85  26.38  80  42-13  29.64 

40  35-82  26.37 


45 


BARIUM    CAPROATB 


BARIUM    CAPROATE  AND  BARIUM    ISO    CAPROATE. 

SOLUBILITY  IN  WATER. 

(Kulisch  —  Monatsh.  Chem.  14,  567,  '93.)  (Konig  —  Monatsh.  Chem.  15,  23,  '94.) 

Barium  Caproate  (Methyl  3  Pentan.)  Barium  Iso  Caproate  (Methyl  2  Pentan.) 

Ba(CH3.CH2CH(CH3)CH2COO)2.  Ba(CH3CH(CH3)CH2.CH2COO)2. 


Gms,Ba(C6Hu02)2 
t<\           per  100  Gms. 

Solid  Phase. 

Water.     Solution. 

0 

11.71 

10 

.49 

Ba(C6Hu02)2.3iH20 

10 

8.38 

7 

•73 

44 

20 

6.89 

6 

•45 

" 

30 

5-87 

5 

•55 

" 

40 

5-79 

5 

•47 

" 

50 

6.63 

6 

.21 

" 

60 

8-39 

7 

•74 

" 

70 

ii  .09 

9 

.98 

" 

80 

14.  71 

12 

.82 

" 

90 

19.28 

16 

.16 

" 

per  100  Gms. 

Solid  Phase. 

Water. 

Solution. 

14-34 

12.54 

Ba(C6HuO2)2.4H3O 

13-33 

11.77 

" 

12  .67 

II  .26 

" 

12.37 

II  .01 

" 

12  .42 

II  .05 

" 

12.83 

11.38 

11 

I3-63 

11.99 

" 

14-68 

12.  80 

" 

16.24 

*3-97 

" 

17-95 

15-23 

** 

BARIUM    CARBONATE     BaCO3. 

SOLUBILITY  IN  WATER. 

(Holleman,  Kohlrausch  and  Rose  —  Z.  physik.  Chem.  12,  129,  241,  '93.) 

Electrolytic  conductivity  method  used. 

i  liter  H2O  dissolves  0.016  g.  BaCO3  at  8.8°,  0.022  g.  at  18°,  and 
0.024  g.  at  24.2°. 

SOLUBILITY  OF  BARIUM  CARBONATE  IN  WATER  CONTAINING  CO2. 

The  average  of  several  determinations  at  about  10°,  by  Bineau, 
Lassaigne,  Foucroy  and  Bergmann'is  i.io  gms.  BaCO3  per  liter  water. 
Wagner  (Z.  anal.  Ch.  6,  167,  '67)  gives  7.25  gms.  BaCO3  per  liter  of 
water  saturated  with  CO2  at  4-6  atmospheres  pressure. 


BARIUM    CHLORATE     BaClO3.H2O. 

SOLUBILITY  IN  WATER. 

(Trantz  and  Anschiitz —  Z.  physik.  Chem   56,  238,  '06;  Kremers  —  Pogg.  Ann.  99,  43.  '56;  Tilden  and 
Shenstone  —  Trans.  Roy.  Soc.  34,  '84.) 


Gms.  Ba(C103)2 

t°.          ] 

aer  100  Gms. 

Solution. 

-     2-75 

15.28 

0 

16.90 

-f  10 

21.23 

20 

25.26 

25 

27-53 

Gms.  Ba(ClO3)2 
t°.       per  TOO  Gms. 
Solution 

30 

29  43 

40 

50 
60 

33  -16 
36.69 
40.05 

70 
80 

43-04 
45-90 

90 

99 
105 
116 
146 


Gms.  Ba(ClO3>a 
per  zoo  Gms. 
Solution. 

48.70 

:     51'-1? 
52.62 

66.0 
78.0 


BARIUM    CHLORIDE  46 

BARIUM    CHLORIDE     BaCl2.2H2O. 

SOLUBILITY  IN  WATER. 

(Mulder;  Engel  —  Ann.  chim.  phys.  [6]  13,  372,  '88;  Etard  —  Ibid.  [7]  2,  535,  '94.) 


AO      Gms.  BaCb  per  100  Gms. 

t     * 

Gms.  BaCl2 

per  100  Gms. 

t   • 

Water. 

Solution. 

Water. 

Solution. 

o 

31.6 

24.0 

60 

46.4 

31-3 

10 

33-3 

25.0 

70 

49-4 

33-i 

20 

35-7 

26.3 

80 

52-4 

34-4 

25 

37-o 

27.0 

100 

58.8 

37-o 

30 

38.2 

27.7 

130 

59-5 

37-3 

40 

40-7 

28.9 

160 

63.6 

38-9 

50 

43-6 

30-4 

2I5 

75-9 

43  -1 

Sp.  Gr.  of  solution  saturated  at  o°  =  1.25;  at  20°  =  1.27. 

SOLUBILITY  OF  MIXTURES  OF  BARIUM  CHLORIDE  AND  BARIUM  NITRATE 

IN  WATER. 
Both  salts  present  in  solid  phase. 

(Etard.) 

Grams  per  100^  Gms.  Solution.  Grams  per  loo^Gms.  Solution. 

BaCl2.  Ba(N03)2.  BaCl2.         *  Ba(NO3)2. 

o  22.5  4.3  ioo  31  14 

20  24.5  6.0  140  32  20 

40  26.5  7.5  180  33  26 

60  28.5  9.5  210  32  32 

SOLUBILITY  OF  MIXTURES  OF  BARIUM  CHLORIDE  AND  MERCURIC 
CHLORIDE  IN  WATER. 

(Foote  and  Bristol  —  Am.  Ch.  J.  32,  248,  '04.) 

Gms.  per  too  Gms.  .  Gms.  per  ioo  Gms. 

t°  Solution.  Solid  t0  Solution.  Solid 

BaCl2.    '   HgU2:  BaCl2.     '      Hgd,. 


10.4     23-58     50-54  {BaSS°+  10.4      22.10     51-66 

10.4       23.44       50-74    (DoubleSalt  IO'4        21.64       5  1-74 

I0.4       22.58       51.23       BaCl2.3HgCl2.  25  23.02       54>83 

10.4       22.48       51.41     ( 

SOLUBILITY  OF  MIXTURES  OF  BARIUM  CHLORIDE  AND  POTASSIUM 
CHLORIDE  IN  WATER. 

(Foote  —  Am.  Ch.  J.  32,  253,  '04.) 

ioo   grams  saturated  solution  contain  13.83   grams    BaCl2  +  18.97 
grams  KC1  at  25°. 

SOLUBILITY   OF   MIXTURES    OF   BARIUM   CHLORIDE   AND   SODIUM 
CHLORIDE  IN  WATER. 

(Precht  and  Wittgen  —  Ber.  14,  1667,  '81;  Rudorff  —  Ber.  18,  1161,  '85.) 

0                Gms.  per  ioo  Gms.  H2O.  Gms.  per  ioo  Gms.  Solution. 

'BaCl2.                NaCl.  BaCl2.                 NaCf. 

20                    4-1                  33.8  2-9                  25.0 

40                    6.3                  33.6  4.5                  23.0 

60  9.7  33.5  6.8  23.4 

80  13.9  33.6  9.4  22.8 

IOO  17.9  33.6  II.  8  22.2 


47  BARIUM    CHLORIDE 

SOLUBILITY  OF  BARIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP 
HYDROCHLORIC  ACID  AT  o°. 

(Engel  —  Ann.  chim.  phys.  [6]   13,  371,  '88.) 


'HCl. 

iBaC!2. 

HCl. 

BaCl2. 

HCl.         BaCl2. 

O 

28 

-90 

O 

30 

.10 

O 

24.07 

I 

.1 

27 

.80 

O 

.40 

28 

•95 

0 

•32 

23 

•31 

2 

.8 

26 

.07 

I 

.02 

27 

•15 

o 

•83 

22 

.11 

5 

.0 

23 

•  40 

I 

.82 

24 

•36 

I 

•51 

2O 

.14 

14 

•4 

14.00 

5 

.24 

14 

•57 

4 

•58 

12 

.76 

18 

.8 

IO 

-20 

6 

.84 

10 

•47 

6 

•J3 

9 

•37 

22 

•7 

6 

.67 

8 

•99 

6 

•95 

h 

•55 

6 

•33 

32 

.0 

2 

•74 

ii 

.66 

2 

•85 

IO 

.81 

2 

.64 

50-5 

0 

.29 

18 

.41 

O 

•3o 

16.92 

O 

.28 

Sp.  Gr.  of  TO  cc   Sol     "          Gms-  I**  ioo  cc.  Sol.        Gms.  per  ,00  g.  Sol. 

Solutions. 

1.250 
1.242 
1.228 
.2IO 

•143 
.Il8 
.099 
.079 
.088 

Less  than  i  part  of  BaCl2  is  soluble  in  20,000  parts  of  concentrated 
HC1  and  in  120,000  parts  of  cone.  HC1  containing  £  volume  of  ether. 

(Mar  — Am.  J.  Sci.[3]  43,  521,  '92-) 

SOLUBILITY   OF   BARIUM   CHLORIDE   IN   ABSOLUTE   METHYL  ALCOHOL 
AND  IN  GLYCERINE. 

(In  Alcohol,  de  Bruyn  —  Z.  physik.  Chem.  10,  783,  '92.) 

ioo  parts  of  CH3OH  dissolve  2.18  parts  BaCl2  at  15.5°,  and  7.3  parts 
BaCl2.2H20  at  6°. 

ioo  parts  by  weight  of  glycerine  dissolve  10  parts  of  BaCl2  at  15.5°. 

SOLUBILITY  OF  BARIUM  CHLORIDE  IN  AQUEOUS  ETHYL  ALCOHOL  AT  15°. 

(Schiff  —  Liebig's  Ann.  118,  365,  '61;  Rohland  —  Z.  anorg.  Ch.  15,  412,  '97.) 

Wt.  per  cent  alcohol      10  20  30  40         60         80          97 

Gms.  BaCl2.2H2Oper 

ioo  g.  aq.  alcohol     31-1       21.9       14.7       10.2       3.5       0.5       0.014 

BARIUM    CHROMATE      BaCrO4. 

SOLUBILITY  IN  WATER  AND  IN  SALT  SOLUTIONS. 


f.  Solvent. 

(  (Kohlrausch  &  Rose  — 

18  Water  0.0038  {  z.  physic.  Ch.  12,  241, 

(  '93-) 

ord.  temp.  o  .  0062  (ignited  BaCrO4)  (  (Schweitzer  -  z.  anal. 

ord.  temp.  o.oioo  (not  ignited)         jch.  20,  4i4,  '90.) 

K     nf  "  0^/1-7  (  (Mescherzerski  —  Z. 

D-  PL  o  .043  j  anah  ch  2I>  39Q7  ,82  } 

Ord.  temp.       I  .5%  Am.  Acetate  0.020  (  (Fresenius  -  Z.     anal. 

ord.  temp.     0.5%  Am.  Nitrate  0.022  jch.ag,  4i8,  'oo-) 

BARIUM    CITRATE     Ba3(C6H5O7)2.7H2O. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

TOO  grams  water  dissolve  0.0406  gram  Ba3(CGH5O7)2.7H2O  at  18°, 
and  0.0572  gm.  at  25°. 

ioo  grams  95%  alcohol  dissolve  0.0044  gram  Ba3(C6H5O7)2.7H2O  at 
18°,  and  0.0058  gm.  at  25°. 

(Partheil  and  Hiibner  —  Archiv.  Pharm.  241,  413,  '03.) 


BARIUM    CYANIDE  48 

BARIUM    CYANIDE     Ba(CN)2. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL  AT  14°. 

(Joannis  —  Ann.  chim.  phys.  [5]  26,  489,  '82.) 

ioo  parts  water  dissolve  80  parts  Ba(CN)2. 

100  parts  70%  alcohol  dissolve  18  parts  Ba(CN)2. 

BARIUM  FERROGYANIDE  AND  BARIUM  POTASSIUM  FERRO- 

CYANIDE. 

(Wyrouboff  —  Ann.  chim.  phys.  [4]  16,  292,  '69.) 

ioo  parts  water  dissolve  o.i  part  Ba2Fe(CN)6.6H2O  at  15°,  and  i.o 
part  at  75°. 

ioo  parts  water  dissolve  0.33  part  BaK2Fe(CN)6.5H2O  at  ord.  temp. 

BARIUM    FLUORIDE     BaF2. 

(Kohlrausch  —  Z.  physik.  Chem.  50,  365,  'o4-'o5.) 

i  liter  of  water  dissolves  1.63  gms.  BaF2  at  18°.     Electrolytic  conduc- 
tivity method. 

BARIUM    FORMATE     Ba(HCOO)2.2H2O. 

SOLUBILITY  IN  WATER. 

(Krasnicki  —  Monatsh.  Chem.  8,  597,  '87.) 

to      Gms.Ba(HCOO)2periooGms.  to       Gms.  Ba(HCOO)2  per  ioo  Gms. 

Water.  Solution.  Water.  Solution. 

o  27.76  21.72  40  34-8i  25.82 

10  28.46  21.15  5°  37 •I4  27.10 

20  30.11  23.15  60  38.97  28.03 

25  31.20  23.80  70  39.95  28.54 

30  32-34  24.45  80  39 .71  28.42 

BARIUM    HYDROXIDE     Ba(OH)2. 

SOLUBILITY  IN  WATER.     SOLID   PHASE  Ba(OH)2.8H2O. 

(Rosenthiel  and  Riihlmann  —  Jahresber.  Chem.  314,  '70.) 

to      Gms.  Ba(OH}2  per  ioo  Gms.  to          Gms.  Ba(OH)2  per  ioo  Gms. 

Water.         Solution.  Water.  Solution. 

o  1.67  1.65  30  5.59  5.29 

5  1.95  1.92  40  8.22  7.60 

10  2.48  2.42  50  13-12  ii. 61 

15  3.23  3.13  60  20.94  17.32 

20  3.89  3.74  75  63.51  38.85 

25  4.68  4.47  80  101.40  50.35 

SOLUBILITY  OF  BARIUM  HYDROXIDE  IN  AQUEOUS  ACETONE  AT  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  41,  321,  '04.) 

_       ,  „  .  „      Ba(OH)2  per  too  cc.  Sat.  Gms.  Ba(OH)2 

Sp.  Gr.  of  Vol.%  Solution.  per 

Solutions.  Acetone. • ,  ioo  Gms. 

Millimols.  Grams.  Solution. 

1.0479  °  55-°8  4-722  4-506 

i. 0168  10  31-84  2.730  2.686 

0.9927  20  17.79  i-525  J-536 

°-9763  3°  9-Jo  o-779  0.798 

0.9561  40  4.75  0.407  0.426 

0-9398  50  1.54  0.132  0.141 

0.9179  60  0.48  0.041  0-045 

0.8956  70  0.08  0.007  0.018 


49  BARIUM    IODATE 

BARIUM    IODATE     Ba(IO3)2.H2O. 

SOLUBILITY  IN  WATER. 

(Trantz  and  Anschiitz  —  Z.  physik.  Chem.  56,  238,  '06.) 

to  Gms  Ba(lp3)2per  t«         Gms.  Ba(IO3)  per  te        Cms.  Ba(IOs)2  per 

100  Gms.  Solution,  100  Gms.  Solution.  100  Gms.  Solution 

—    0-046  O.OOS  30  O-O3I  7O  0-093 

+  10       0.014       40     0.041        80     0.115 

2O         O-O22          50       0-056  QO       O.I4I 

25       0.028       60     0-074       ioo     0.197 

BARIUM    IODIDE     BaI2. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg.  Ann.  103,  66,  1858;  Etard  —  Ann.  chim.  phys.  [7]  2,  544,  '94.) 
Gms.  BaI2  per  ioo  Gms.  Gms.  BaI2  per  ioo  Gms.  0 

Water.     Solution.         Solld  Phase'  *•       Water,     'solution.       ***  ^^ 

-20     143-9    59-o    BaI2.6H2O          40    231.9    69.8    BaI2.2  H2O 
o     170.2     63.0  60    247.3     71-2  " 

4-10     185.7     65.0  80    261.0    72.3  " 

20    203.1     67.0  ioo    271.7     73.1  " 

25     212.5     68.0  120    281.7     73-8  " 

30     219.6     68.7  160     294.8     74.6  " 

Sp.  Gr.  of  saturated  solution  at  19°. 5  =  2.24. 

For  method  of  interpolating  above  results,  see  Note,  page  33. 

ioo  grams  97%  Ethyl  Alcohol  dissolve  1.07  g.  BaI2.2H2O  at  15°. 

(Rohland  —  Z.  anorg.  Chem.  15,  417,  1897.) 

BARIUM    MALATE     BaC4H4O6. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Basadonna  —  Bull.  soc.  chim.  [3]  35,  731,  '06.) 

to       Gms.BaQHiOg  .0       Gms.BaC4H4O5  -0      Gms.EaC^Os 

per  ioo  cc.  Sol.  per  ioo  cc.  Sol.  per  ioo  cc.  SoL 

20    0.883       35    0.895       60    i.  oi  i 
25     0.901       40    0.8        70    1.041 

30      0.903         50     0.942         80      1.044 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Rartheil  and  Hiibner  —  Archiv.  Pharm.  241,  413,  '03.) 

ioo  grams  water  dissolve  1.24  gms.  BaC4H4O6  at  18°,  and  1.3631 
gms.  at  25°. 

too  grams  95%  alcohol  dissolve  0.0038  gms.  BaC4H4O6  at  18°,  and 
0.0039  Sm-  at  25°. 

BARIUM    MALONATE     BaC3H2O4.N2O. 

SOLUBILITY  IN  WATER. 

(Miczynski  —  Monatsh.  Chem.  7,  263,  '86.) 

0  Gms.BaC3H2O4per  looGms.  0        Gms.  BaC3H2O4  per  ioo  Gms. 

Water.  Solution.  Water.  Solution. 

o       0.143    0.143       50    0.287    0.285 
10       0.179    0.179       60    0.304    0.303 

2O         O-2I2     O-2II  7O     0.317     0.316 

30         0.241     0.240  80     0.326     0-325 

40  o -  266         o . 265 

BARIUM    MOJ.YBDATE     BaMoO4. 

ioo  parts  water  dissolve  0.0058  part  BaMoO4  at  23°. 

(Smith  and  Bradbury  —  Ber.  24*  2930,  '91. ^ 


BARIUM    NITRATE  50 

BARIUM    NITRATE     Ba(NO3)2. 

SOLUBILITY  IN  WATER. 

(Mulder;  Gay  Lussac;  Etard  —  Ann.  chim.  phys. [7]  2,  528,  94;  Euler  —  Z.  physik.  Chem 


Gms.  Ba(NO3)2 
•jo                    per  100  Gms.                            t°. 

Gms.  Ba(N03)2 
per  loo  Gms. 

Water. 

Solution. 

'Water. 

Solution. 

O 

5-o 

4.8 

80 

27.0 

21.3 

10 

7-o 

6-5 

100 

34-2 

25-5 

20 

9.2 

8.4 

120 

42.0 

29.6 

25 

10.4 

9-4 

I4O 

5O-O 

33-3 

30 

ii.  6 

10.6 

160 

58.0 

36-7 

40 

14.2 

12.4 

180 

67.0 

40.1 

5° 

17.1 

14.6 

200 

76.0 

43-2 

60 

20.3 

16.9 

215 

84-5 

45-8 

Sp.  Gr.  of  saturated  solution  at  19.5°  =  1.072. 


SOLUBILITY  OF  MIXTURES  OF  BARIUM  NITRATE  AND  LEAD  NITRATE 
IN  WATER  AT  25°. 

(Fock.  —  Z.  Kryst.  Min.  28,  365,  '97;  at  17°,  Euler  —  Z.  phyisk.  Chem.  49,  315,  '04.) 


J.I1    OOIUUOU. 

In  Solid  Phase. 

3.  Gr.  of 
>olution. 

Gms. 

per  Liter. 

Mg.  Mols. 

per  Liter. 

Mol.  % 

Mol.% 
Ba(NfV)o 

Ba(N03)2. 

Pb(N03)2. 

Ba(N03)2. 

Pb(N03)2 

Ba(N03)2. 

r><i\iM  v^3/2 

1.079 

102.2 

O 

391.0 

O 

100 

IOO 

I  .088 

54-9 

17.63 

210.  I 

53-3 

79.78 

98.30 

I.IOS 

86.5 

49.80 

330-7 

J5o-7 

68.70 

96.74 

I.II9 

79-7 

68.10 

304-9 

205.7 

59-69 

94-80 

I  .I4O 

77.0 

97.20 

294-4 

293.6 

50.09 

93.62 

.163 

69.8 

130.7 

266.8 

395-o 

40.31 

92.49 

.198 

66.0 

177-3 

252-S 

535  -6 

32-03 

90.07 

.252 

57-5 

247-7 

222  .6 

748.5 

22  .91 

83-47 

.294 

25-9 

334-3 

99-2 

1010.3 

8.  II 

75-44 

•376 

28.8 

429.7 

110.3 

1298.0 

7-77 

35-11 

1.459  ...         553-8  o.o       1673.0  o.o  o-o 

Tables  of  results  are  also  given  for  15°,  30°,  and  47°. 


SOLUBILITY  OF  MIXTURES  OF  BARIUM  NITRATE  AND  POTASSIUM 
NITRATE  IN  WATER  AT  25°. 

(Foote  —  Am.  Ch.  J.  32,  252,  '04.) 


Per  IPO  Grams  Solution. 

Grams  Solid  Phase. 

Gms.  KN03.        Ba(N03)2. 

14-89  6 .62  Ba(NO3)2  and  2  KNO3.Ba(NO3;2 

J6  -30  5  -49  1  Double  salt, 

21  99  3  .04  j  2  KNO3.Ba(NO3)2 

27 . 76  2 .04  KNO3  and  2  KNO3.Ba(NO3)2 


5i  BARIUM    NITRATE 

SOLUBILITY  OF   BARIUM   NITRATE  IN   AQUEOUS   PHENOL   SOLUTIONS 

AT   25°. 

(Rothmund  and  Wilsmore  —  Z.  phyisk.  Chem.  40,  620,  '02.) 


G.  Mols. 

per  Liter. 

Gms.  per  Liter. 

G.  Mols.  per  Liter. 

Gms.  per  Liter. 

C«H6OH 

Ba(N03)2. 

C8H6OH. 

Ba(N03)2. 

C6H6OH 

Ba(N03)2. 

C8H6OH.  Ba(NOa)2. 

O-OOO 

o-3835 

O 

.0 

IOO 

.2 

o 

.310 

0.3492 

29 

.12 

9I-3I 

0.045 

0-3785 

4 

23 

98 

•97 

o 

.401 

0.3400 

37 

•73 

88.90 

0-082 

0.3746 

7- 

71 

97 

95 

o. 

501 

0.3299 

47 

.11 

86.26 

0.146 

0.3664 

13 

73 

95 

.81 

o 

.728 

(sat.)  0.3098 

68 

•45 

81.00 

BARIUM    NITRITE     Ba(NO2)2.H2O. 

SOLUBILITY  IN  WATER. 

(Vogel  —  Z.  anorg.  Chem.  35.  389,  '03.) 


20' 


Gms.  Ba(NO2)2  per  100  gms.  H2O   58    63 


25 


82 


35° 
97 


BARIUM  OXALATE     BaC2O4. 

SOLUBILITY  OF  THE  THREE  HYDRATES  IN  WATER. 

(Groschuff  —  Ber.  34,  3318,  '01.) 


BaC2043*H20. 


BaC2O4.2HoO. 


BaC204.£H2O. 


t°.    Gms.BaC2O4   G.M.BaC2O4 

Gms.BaC2O4 

G.  M.  BaC2O4 

Gms.BaC2O4 

G.  M.  BaC2O4 

per 

per  loo  Mol. 

per 

per  loo  G.  M. 

per 

per  loo  Mol. 

1000  g.  Sol. 

H20. 

1000  g.  Sol. 

H20. 

1000  g.  Sol. 

H2O. 

0 

0.058 

o  .  00046 

0-053 

0.00042 

0-089 

O.OOO7O 

9 

•5       0.082 

O.OO066 

18 

O.II2 

O.OOO9O 

0-089 

O.OOO7I 

O.I24 

0.00099 

30 

0.170 

0-00136 

O-I2I 

0.00097 

O.I4O 

O.OOII2 

40 

0.152 

O.OOI22 

O.I5I 

O.OOI2I 

45 

0.169 

0.00135 

55 
60 

65 
73 
75 
90 

IOO 


O.2I2     O.OOI7O 


0.164     O.OOI3I 
O.I75     O.OOI4O 


0.250 
0.285 


O.OO2OO 
O.OO228 


0.188 

O.2OO 
O.2II 


O.OOI5I 
O.OOl6o 
0.00169 


SOLUBILITY  OF  BARIUM  OXALATE  (BaC2O4.iH2O)  IN  AQUEOUS 
ACETIC  ACID  AT  26°-2j°. 

(Herz  and  Muhs.  —  Ber.  36,  3715,  '03.) 
lity    G.  Residue*  Gms-  P61"  ioocc.  Solution.    Normality     G.  Residue*     G ms. per  100  cc.  Solution 


of  Acetic 
Acid. 

per  50.05  cc. 
Sol. 

CHsCOOH.  Ox^fate> 

of  Acetic 
Acid. 

per  50  cc. 
Sol. 

CHsCOOH. 

Ba  Oxalate 

O 

O 

.0077 

o.oo 

0.0154 

3- 

85 

O 

.0564 

23' 

12 

O.II27 

o-565 

0 

•0423 

3-39 

o  .  0845 

5- 

79 

0 

.O5II 

34 

76 

0-I02I 

1.425 

o 

.0520 

8-55 

o  .  1039 

i7- 

3o 

O 

.0048 

103 

.90 

0-0096 

2.85 

0 

•0556 

17.11 

O-IIII 

*  Dried  at  70°. 

BARIUM    ACID    OXALATE         52 

BARIUM    ACID    OXALATE     BaC2O4.H2C2O4.2H2O. 

SOLUBILITY  IN  WATER. 

(Groschuff.) 


A0      Gms.  per  100  Gms.  Solution. 

Mols.  per  100  Mols.  H2O. 

Mols.  H2C 

V      * 

H2C204. 

BaC2O4. 

H2C204. 

BaC2O4.       Per  i  MoLBa 

0 

0.27 

0.030 

0.054 

0.0024 

22 

18 

0.66 

O.O7O 

0.130 

0.0056 

24 

20.5 

0.76 

0.076 

0.15 

0.0061 

25 

38 

1.61 

0.16 

o-33 

0.013 

25 

4i 

1.82 

0.18 

0.37 

0.015 

25 

S3 

2.92 

0.31 

0.60 

O.O26 

24 

60 

3.60 

0.40 

o-75 

0.033 

22-5 

80 

6.21 

0.81 

i-34 

0.070 

J9 

90 

7.96 

i  .11 

i-7S 

0-098 

18 

99 

10.50 

i-55 

2-39 

O.I4I 

J7 

BARIUM    PROPIONATE     Ba(C3H5O2)2.H2O.  also  6H2O. 
SOLUBILITY  IN  WATER. 

(Krasnicki  —  Monatsh.  Chem.  8,  597,  '87.) 


t°. 

Gms.] 
per 

ioo  Gms. 

Water. 

Solution. 

o 

47-98 

32.41 

10 

51  .56 

34-02 

20 

54-82 

35-42 

30 

57-77 

36-65 

40 

60.41 

37.66 

Gms.  Ba(C3H3O2)2 
t°.                         per  lop  Gms. 

50 
60 
70 
80 

Water. 
62.74 
64.76 
66.46 
67.85 

Solution. 
38.57 

39  -31 
39-93 
40.42 

BARIUM    SULPHATE     BaSO4. 

SOLUBILITY  IN  WATER. 
Electrolytic  Conductivity  Method. 

(Holleman;  Kohlrausch  and  Rose  —  Z.  physik.  Chem.  12,  131,  241,  '93.) 


t 


iov 


26° 


34C 


37-7' 


Gm.  BaSO4  per  liter    0.0017     0.0020    0.0023     0.0026    0.0029     0.0031 

SOLUBILITY  OF  BARIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC AND  OF  NITRIC  ACIDS. 

(Banthisch  —  J.  pr.  Chem.  29,  54,  1884.) 

In  Hydrochloric  Acid.                                                            In  Nitric  Acid. 
, * x         , *• N 

cc.  containing  Mgs.  BaSO4        Gms   per  100  cc.    Cc.  containing    Mgs.  BaSO4          Gms.  per  100  cc. 
i  Mg.Equiv.  per  i  Mg.  Equiv.  Solution.  i  Mg.Equiv.  per  i  Mg.Equiv.  Solution. 

ofHCl.  ofHCl.  gel BaS04:        of  HNO3.        of  HNO3.  HNO3.        BaSO4. 

2.0  0.133  1.82  0.0067  2.0  0.140  3-I5  0.0070 
i.o  0.089  3-65  0.0089  i.o  0.107  6.31  0.0107 
0.5  0.056  7-29  o.oioi  0.5  0.085  12. 61  0.0170 

0.2      0.017    18.23   0.0086     0.2     0.048     3I-52   0.0241 

TOO  cc.  HBr  dissolve  0.04  gms.  BaSO4;  100  cc.  HI  dissolve  0.0016 
gms.  BaSO4  at  the  boiling  point. 

(Haslam  —  Chem.  News  53,  87,  '86.) 


53  BARIUM    SULPHATE 

SOLUBILITY  OF  BARIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  IRON, 
ALUMINUM  AND  MAGNESIUM  CHLORIDES  AT    20°  —  25°. 

(Fraps.  —  Am.  Ch.  J.  27,  290,  '01.) 

Gms.              Milligrams  BaSO4  per  Liter  in:  Gms.  Mgs.  BaSO4  per  Liter  in: 

Chloride       , * s  Chloride 


per  Liter.    Aq.  FeCl8.    Aq.  A1C13.    Aq.  MgCl2.        per  Liter.  Aq.  FeCl3.    Aq.  A1C13.    Aq.MgCl2. 

i  58  33  30  25  150  116  50 

2\  72  43  30  50  160  170  50 

5  IJ5  6o  33  ioo  170  175  50 

10  123  94  33 

BARIUM    PerSULPHATE     BaS2O8.4H2O. 

100  parts  water  dissolve  39.1  parts  BaS2O8  or  52.2  parts  BaS2O8. 
4H2O  at  o°. 

(Marshall  — J.  Ch.  Soc.  59,  771,  '91. 

BARIUM    SULPHITE     BaSO3. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Rogowicz  —  Z.  Ver  Zuckerind.  938,  1905.) 


Cone,  of 

Gm.  BaSU, 

i  per  100  cc.  bol. 

Cone,  of 

Gm.  BaSO4  per 

100  cc.  Sol. 

Sugar  Sol. 

at  20°. 

at  80°. 

Sugar  Sol. 

at  20°. 

at  80°. 

o°Bx 

0.0197 

0.00177 

40°  Bx 

o  .  0048 

0.00158 

10°     " 

O-OIO4 

0-00335 

50°   " 

0.0030 

O.OOI49 

20°     " 

0.0097 

0-00289 

60°   "  (sat.) 

0.0022 

O-OOII2 

30°    " 

O.OO78 

o  .00223 

BARIUM    SUCCINATE  AND  BARIUM  ISO  SUCCINATE 

Ba.CH2CH2(COO)2.  Ba.CH3CH2(COO)2. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Miczynski  —  Monatsh.  Chem.  7,  263,  1886.) 

Gms.  Ba.  Succinate  Gms.  Ba.  Iso  Succinate 

t°.  per  100  Gms.  per  100  Gms. 

Water.  Solution.  Water.  Solution. 

o  0.421  0.420  1.884         1-849 

10  0.432  0.430  2.852         2.774 

20  0.418  0.417  3-6i8        3-493 

30  0.393  0.392  4.181         4.014 

40  0.366  0.365  4-542         4-346 

50  0.337  0.336  4.700         4-594 

60  0.306  0.305  4-656        4-450 

70  0.273  0.272  4.410        4.224 

80  0.237  0.237  3-962         3-8l° 

100  gms.  H2O  dissolve  0.396  gms.  Ba  Succinate  at  18°  and  0.410 
gms.  at  25°. 

100  gms.  95%  alcohol  dissolve  0.0015  gms.  Ba  Succinate  at  18°  and 

0.00 1 6  gms.  at  25°.  (Partheil  and  Hiibner—  Archiv.  Pharm.  241,  413.  '03-) 

BARIUM    TARTRATE     Ba(C2H2O3)2. 

SOLUBILITY  IN  WATER. 

(Cantoai  and  Zachoder  —  Bull.  soc.  chim.  [3]  33,  751,  '05;  see  also  Partheil  and  Hiibner.) 


Gms.  Ba(C2H2O3)2 
t°.              per  100  cc.                 t°. 

Gms.  Ba(C2H2O3)2 
per  100  cc. 

t\ 

Gms.  Ba(C2H2 
per  100  cc. 

Solution. 

Solution. 

Solution. 

0 

O.O2O5 

30 

0.0315 

70 

o  .  0480 

10 

0.0242 

40 

0.0352 

80 

0.0527 

2O 

O.O279 

50 

0-0389 

90 

0.0541 

25 

0.0297 

60 

0.0440 

•• 

BARIUM    TARTRATE  54 

SOLUBILITY  OF  BARIUM  TARTRATE  IN  AQUEOUS  ACETIC  ACID 
SOLUTIONS  at  26°-27°. 

(Herz  and  Muhs  —  Ber.  36,  3715,  '03.) 

Normality  Gms.  residue*  G ms. per  loocc.  Solution.  Normality.  Cms.  residue*  Gms. per  icocc.  Solution 
°fAcfdtiC       ^Vol."       CHaCOOH.'Ba  tartrate;    °^IC         ^f. CC'     CH3COOH:  Ba  tartrate'. 

o  0.0328  o.o  0.0655  3-77  0.1866   22.62   0.3728 

0.565  0.1151  3.39  0.2300    5.65  0.1865   33.90   0.3726 

1.425  0.1559  8.55  0.3115  16.85  0.0218  101.10   0.0436 

2.85  0.1739  17.11  0.3475    •••     

*  Dried  at  70°. 

ioo  grams  95%  alcohol  dissolve  0.032  gm.  Ba  tartrate  at  18°  and 

0-0356  Sm-  at  25°-  (Partheil  and  Hiibner.) 

BENZALDEHYDE     C6H5COH. 

ioo  gms.  H2O  dissolve  0.3  gm.  benzaldehyde  at  room  temperature. 

(Fluckiger  —  Arch.  Pharm.  [3]  7,  103,  '75.) 

BENZAMIDE     C6H6CONH2. 

SOLUBILITY  IN  ETHYL  ALCOHOL. 

(Speyers  — Am.  J.  Sci.  [4]  14,  295,  '02.) 


G.M.                 Gms. 
to    Sp.  Gr.  of    C6H6CONH2      C6H8CONH2       to 
'     Solutions,     per  ioo  G.M.     per  ioo  Gms. 
CjjHsOH.          C2HsOH. 

Sp.  Gr.  of 
Solutions. 

G.M. 
C6H6CONH2 
per  ioo  G.M. 
C2H6OH. 

Gms. 
C6HSCONH2 
per  ioo  Gms. 
CgHsOH. 

O 

3.833 

3 

,i 

8 

•J5 

40 

0.848 

II  . 

O 

28 

.92 

10 

0.832 

4 

2 

ii 

.04 

5o 

0.862 

14. 

2 

37 

•34 

2O 

0.833 

D 

9 

I5 

•52 

60 

0.881 

17 

2 

45 

.22 

25 

0.835 

6 

.8 

*7 

.87 

70 

0.913 

20. 

4 

•63 

30 

0.838 

8 

.2 

21 

•56 

.  . 

. 

.  . 

SOLUBILITY  OF  BENZAMIDE  IN  MIXTURES  OP  ALCOHOL  AND  WATER 


AT  25 


(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  294,  '94.) 


Vol. 
A 


Gms. 

Gms. 

CBH6CONH2 

per  ioo  Gms. 

Sp.  Gr.  of 
Solutions. 

Vol.% 
Alcohol. 

QjHeCONHa 
per  ioo  Gms. 

Sp.  Gr.  of 
Solutions. 

Solvent. 

Solvent. 

17.03 

0.830 

70 

23.87 

0.925 

21  .12 

0.856 

60 

18.98 

0-939 

24.50 

0.878 

5° 

13-74 

0-949 

26.15 

0-895 

40 

8.62 

0.958 

26.63 

O.9OO 

31 

5-33 

0.967 

26.43 

0.907 

15 

2.28 

0.912 

25.41 

0.917 

O 

J-35 

0.999 

IOO 

95 
90 
85 
83 
80 

75 

BENZENE     C6H6. 

SOLUBILITY  IN  WATER  AT  22°. 

(Herz  —  Ber.  31,  2671,  '98.) 

ioo  cc.  water  dissolve  0.082  cc.  C6H6,  Vol.  of  Sol.  =  100.082, 
Sp.  Gr.  =  0.9979. 

ioo  cc.  C6H6  dissolve  0.211  cc.  H2O,  Vol.  of  sol.  =  100.135, 
Sp.  Gr.  =  0.8768. 


55 


BENZENE 


BENZENE,  ACETIC  ACID,  WATER  MIXTURES. 

(Lincoln  —  J.  Physic.  Chem.  8,  2<;i,  '04.) 

NOTE.  —  To  mixtures  of  known  amounts  of  acetic  acid  and  benzene, 
water  was  gradually  added  until  clouding  occurred.  The  same  degree 
of  clouding  did  not  represent  the  end  point  in  all  cases,  as  was  assumed 

by  Waddel.     (J.  Physic.  Chem.  4,  161,  'oo.) 


At  25°. 


cc. 

cc. 

cc. 

:oo 

H.      C6HC. 

H2O. 

5 

10-  06 

o-45 

5 

8.04 

o-55 

5 

6.03 

0.64 

5 

3.02 

0.98 

5 

2  -OI 

1.28 

5 

I  .01 

1.89 

5 

O.6o 

2.80 

5 

o-35 

4-54 

5 

0.17 

9-53 

At  35°. 


cc. 

cc. 

cc. 

CH3COOH. 

C6H«. 

H20. 

IOO 

iS.IO 

I.I4 

IOO 

16.09 

I  .22 

IOO 

10.  06 

I  .55 

IOO 

6.03 

2.17 

IOO 

4-02 

2-77 

IOO 

3-oi 

3.26 

IOO 

I  .00 

7.01 

IOO 

0.65 

10.10 

IOO 

0.47 

13.64 

BENZENE,  AQ.   ALCOHOL   MIXTURES;   BENZENE,  AQ.   ACETONE   MIX- 
TURES  AT    20°. 

H2O  added  to  mixtures  of  known  amounts  of  the  other  two  and 
appearance  of  clouding  noted. 

(Bancroft  —  Phys.  Rev.  3,  31,  1895. g6.) 

C6H6,C2H5OH and H2O     C6H6,CH3OH and H2O  C6H5,(CH3)2CO  and  H2O 

Per  5  cc.  C2H5OH.  Per  5  cc.  CH3OH.  Per  5  cc.  (CH3)2CO. 


cc.  H20. 

cc.  C6Hfi. 

cc.  H2O. 

cc.  C6H6. 

cc.  H2O. 

cc.  C6H0." 

2O 

0.03 

5-o 

O.I5 

8.0 

O-IO 

8 

o  •  J3 

3-o 

O.2I5 

3-o 

o-395 

4 

o-39 

2  .0 

o-59 

2  .O 

0.69 

2 

1.17 

1.4 

I  -0 

i-3 

I  .0 

I-S 

1.87 

I  .0 

1.9 

0.51 

2  -O 

I  .0 

3-57 

0.8 

3-o 

0.295 

3-o 

0.605 

8.0 

0.69 

4-0 

0.2 

4-0 

o-34 

20.  o 

0.49 

8.0 

o  .  15 

5-o 

MUTUAL   SOLUBILITY   OF   BENZENE   AND  0   NAPHTHALENE    PICRATE 

C6H2(NO2)3OH.C10H7OH. 
"  Synthetic  Method  "  used  —  see  Note,  p.  9. 

(Kuriloff  —  Z.  physik.  Chem.  24,  442,  '97.) 

t       . 

in  .6 

102.0 

29-5 
4-6 

5-02 

a  =  Mols.  /3  Naphthalene    Picrate  per  100    Mols.  of  /3  Napthalene 
Picrate  plus  Benzene. 

Determinations  for  a  large  number  of  isothermes  are  also  given. 


t°. 

Cms. 
Picrate. 

Cms. 
Benzene 

a 

157 

100.0 

IOO.O 

148.4 

2.128 

O.II5 

79-3 

J37-4 

1.274 

0.170 

61.1 

134.2 

1.384 

0.297 

49-3 

126.8 

I  .019 

0-343 

38.3 

Gms. 
Picrate. 

Gms. 
Benzene. 

a 

I-I73 
1.087 

1.037 
1.780 

19.2 
II  .2 

0.390 
1.329 

8.430 
21.  80 

o-95 
0.48 

IOO-O 

BENZENE  56 

SOLUBILITY  OF  BENZENE  IN  SULPHUR. 
By  "  Synthetic  Method,  "  see  Note,  p.  9. 

(Alexejew  —  Ann.  Physik.  Chem.  28,  305,  '86.) 

to     Gms.  C6H6  per  100  Gms.  to  Gms.  C6H6^per  100  Gms. 

S  Layer.  C6H6  Layer!  S  Layer.  C«H6  Layer." 

ioo  6  75  140       16  61 

no  8  72.5  150       19  55 

120  10  70  160       25  45 

130  12  66  164  (crit.  temp.)  35 

Di  Brom  BENZENE  (p)     C6H4Br2. 

SOLUBILITY  IN  ETHYL,  PROPYL,  Iso  BUTYL  ALCOHOLS,  ETC. 

(Schroder  —  Z.  physik.  Chem.  n,  456,  '93.) 

Determinations  by  "  Synthetic  Method"  see  Note,  p.  9. 

Grams  C6H4Br2  (p)  per  ioo  Grams  Sat.  Solution  in: 


t  . 

C2H6OH. 

CgHyOH. 

(CH3)CH.CH2OH. 

(C2H6)20. 

CS2. 

C6H6. 

C6HsBr. 

0 

27 

10 

30 

34 

34 

22 

20 

.  .  . 

38 

43 

43 

29 

30 

14 

.  . 

15 

47 

53 

53 

36 

40 

19 

20 

57 

62 

62 

45 

50 

26 

2,7 

30 

67 

72 

7i 

54 

60 

38 

40 

44 

77 

81 

80 

67 

70 

57-6 

67 

65 

87 

90 

88 

79 

75 

80.5 

85 

77 

84 

80 

94-4 

95 

94.6 

90 

Chlor  BENZENE     C6H5C1. 

SOLUBILITY  OF  CHLOR  BENZENE  IN  SULPHUR. 
"  Synthetic  Method,  "  see  page  9. 

(Alexejew.) 

Grams  CfiHsCl^per  ioo  Grams. 

t°.  Sulphur  Chlor  Beii- 

Layer.  zene  Layer. 

90  13  70 

ioo  18.5  63 

no  27  53 

116  (crit.  temp.)  38 

For  the  solubility  of  Mixtures  of  di  Chlor  Benzene  and  di  Brom 
Benzene  in  aqueous  Ethyl  Alcohol  solutions  see  Thiel. 

(Z.  physik.  Chem.  43,  656,  1003.) 

Di  Nitro  BENZENE  (m)     C6H4(NO2)2. 

SOLUBILITY  IN  BENZENE,  BROM  BENZENE  AND  IN  CHLOROFORM. 
"  Synthetic  Method." 

(Schroder.) 

Gms.  C6H4(NO2)2  per  ioo  Gms.  C6H4(NO2)2  per 

t<\  Gms.  Sol,  in:  t°.  ioo  Gms.  Sol,  in: 


C6H6.  C6H5Br.    CHCla.                                   C6H6.     C6H5Br.    CHC13. 

15       17.5  ...         22.2  40       52.O      38.0      42.O 

20       26.0  18.5       25.0  50      62.5       47.5       52.5 

25     33-o  23-7     29-o  60     71.0     57.0    65.0 

30    40.0  28.7    33.0  ........... 


57 


BENZENES 


Solubilities  of  Di-Nitro  BENZENES  and  of  Tri-Nitro  BENZENES  in 
Several  Solvents. 

(de  Bruyn  —  Rec.  trav.  chim.  13,  116,  150,  '94.) 

Grams  per  too  Grams  Solvent. 


Solvent. 

Methyl  Alcohol 
Ethyl  Alcohol 

20 

20. 

5 
5 

3-3° 
1.9 

(N6°75' 
3-5 

(/OC6H4. 
(N02)2. 
o.  69 
0.4 

(s)C  H 

4-9  (i  6°)   16.2     (15.5°) 
1.9  (16°)     5-  45  (15.5°) 

Propyl  Alcohol 

20.5 

i 

.09 

2 

.4 

o 

298 

Carbon  Bi-Sulphide 

17- 

6 

0 

.236 

I 

•35 

0 

I48 

o 

25 

Chloroform 

17- 

6 

27 

.  I 

32 

•4 

I. 

82 

6 

i 

Benzene 

18. 

2 

5 

.66 

39 

•45 

2. 

56 

6 

2  (16°) 

Ether 

17- 

5 

. 

i 

-5 

t 

Ethyl  Acetate 

18. 

2 

12 

.96 

36 

.27 

3- 

56 

t 

Toluene 

16. 

2 

3 

.62 

3° 

.66 

2. 

36 

t 

Carbon  Tetra  Chloride 

16. 

2 

0 

•143 

i 

.18 

0. 

12 

.  .  . 

f 

Water 

(ord.) 

0 

.014 

0.0525 

0. 

008 

. 

Symmetrical  Tri-Nitro  BENZENE. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  25°. 

(Holleman  and  Antusch —  Rec.  trav.  chim.     13,  296,  '94.) 


Vol.% 
Alcohol. 

r.  C6H3(N03)3(*) 

per  100  g. 
Solvent. 

Sp.  Gr.  of 
Solutions.        . 

Vol.  % 
Alcohol. 

G.  C6H3(N03)3(*) 
per  loo  g. 
Solvent. 

Sp.  Gr.  of 

Solutions. 

100 

2-34 

0-7957 

80 

o-57 

0.8582 

95 

1-57 

0.8131 

75 

0.47 

0-8708 

90 

I  .12 

0.8288 

7o 

0.37 

0.88o8 

85 

o-79 

0.8436 

60 

0.23 

0.9064 

BENZOYL  PHENYL  HYDRAZINE     C6H6.NH.NH.C7H6O. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL. 

(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  291,  '94.) 


Vol.% 
Alcohol 

Gms.  Hydrazine 
per  loo  g. 
Solvent. 

Sp.  Gr. 

Solutions. 

100 

2-39 

0-793 

95 

2-43 

0.814 

93 

3.00 

0.822 

90 

2.26 

0.831 

Vol.  % 
Alcohol. 

Gms.  Hydrazine 
per  100  g. 
Solvent. 

Sp.  Gr. 
Solutions. 

80 
70 

i  59 
i.  08 

0.859 
0-884 

55 
40 

0.51 
0.16 

0.917 
0.946 

BENZO    SULPHONIC    ACIDS. 

SOLUBILITY  IN  WATER. 

(Bahlman  —  Liebig's  Ann.  186,  309,  '77.) 


Name  of  Acid. 

0-Amido  benzo  sulphonic  acid. 
Amido  brom  benzo  sulphonic  acid. 
Mono  brom  amido  benzo  sulphonic  acid. 
Barium  di-brom  benzo  sulphonic  acid. 
Barium  nitro  brom  benzo  sulphonic  acid 

(hydra  ted). 
Barium  nitro  brom  benzo  sulphonic  acid 

(anhydrous). 

*  At  18°  =  i  .201. 


Gms.  Sulphonic  Add  per  100  Gms. 
Solution  at: 


11°  =  1.301 
8°  =  0.737 

12°  =  0.431 
14°  =  1.713 

15°=  1-436 

16°  =  1.131* 
15°  =  0.463 
9°  =  i  ,098 

16°  =  0.527   30°  =  0.914 
8°  =  0.156 


BENZINE  58 

BENZINE     (Petroleum)  C5H12C6H14. 

ioo  parts  of  alcohol  dissolve  about   16  parts  benzine  of  0.638  — 
0.660  Sp.  Gr.,  at  25°. 

BENZOIO    ACID     C6H6COOH. 

SOLUBILITY  IN  WATER. 

(Bourgoin  —  Ann.  chim.  phys.  [5]  15,  171,  '78.) 

Grams.  C6H6COOH  Grams.  CflH8COOH 

^o^  per  ioo  Gms.  t°.  per  ioo  Gms. 

Water.  Solution.  Water.  Solution. 

o      0.170   0.170       40      0.555    0.551 

10          0.210     0.209  50          0-775     0.768 

20  0.290        0.289  60  I-I55         1.142 

25  0.345        0.343  80  2.715        2.643 

30  0.410        0.408  ioo  5.875        5.549 

ioo    grams    saturated    aqueous    solution    contains     0.340     gram 
C6H5COOH  at  25°;  0.353  gram  at  26.4°;  0.667  gram  at  45°- 

(Paul—  Z.  physik.  Ch.  14,  in,  '94;  Noyes  and  Chapin  —  Ibid.  27,  443.  '98 

Ibid.  51,  393,  '05;   Philip  —  J.  Ch.  Soc.  87,  992,  '05  ;   see  also  Alexeje\v 

305,  '86;  Ost  — J.pr.  Ch.[2]  17,  232,  '78;  Vaubel  —  Ibid. la] 

SOLUBILITY  OF  MIXTURES  OF  LIQUID  BENZOIC  ACID  AND  WATER. 

(Alexejew.) 

Determinations   by"  Synthetic   Method,"  see   Note,  p.  9.     Figures 
read  from  curve. 

Gms.  CfiH5COOH  per  ioo  Gms.  Gms.  C6H5COOH  per  ioo  Gms. 

Aq.  Layer.     Benzoic  Ac.  Layer.  Aq.  Layer.  Benzoic  Ac.  Layer. 

70        6  83  ioo  12.0  69.0 

80        7.5  79.5  no  18.0  59.0 

90        8.5  76  116  (crit.  temp.)    35 

SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF: 

(Hoffman  and  Langbeck.) 

Potassium  Chloride  at  25°.  Potassium  Nitrate  at  25°. 


es  and  Chapin  —  Ibid.  27,  443,  '98;  Hoffman  and  Langbeck  — 
see  also  Alexejew  —  Ann.  Phys.  Ch.  28, 
52,  73,  '95.) 


Nor- 
mality 

Gms. 
KC1. 

Dissolved  QHsCOOH.               ^JJ"           ^gg; 

Dissolved  C6H5COOH. 

of  Aq. 
KC1. 

Liter. 

Mol  .  Cone  .       Wt  .  per  cent  .            -j^J 

Liter. 

Mol.  Cone.        Wt.  per  cent. 

O.O2 

1.49 

5 

0254-10-* 

0. 

339 

0.02 

2 

.02 

5 

.0326-IO~~4 

0.340 

0.05 

3-73 

4 

.9801      " 

o. 

333 

O.O5 

5 

.06 

r 

.0421       " 

0.341 

O.2O 

14.92 

4 

7639      " 

o. 

322 

0.20 

20. 

24 

5 

0297       « 

0.340 

0.50 

37-3° 

4. 

3632      " 

o. 

295 

0.50 

5° 

59 

4 

.9400 

o-334 

1.  00 

101  . 

19 

4 

.7646       " 

0.322 

SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF: 

(Hoffmann  and  Langbeck.) 


Nor- 
mality 

nf  An 

Sodium  Chloride. 

Gms.             Gms.  CfiH5COOH 
NaCl             per  ioo  Gms.  Sol. 

Sodium  Nitrate. 

^rT~              J^™            Gms-  C6H5COOH 
mahty               NaNO3            per  I00  Gms.  g^ 

OI  AC]. 

NaCl. 

JT 

Cl 

at 

2S°- 

at  45°- 

oi  AQ. 
NaN03. 

JJC1 

Liter. 

at  25°.' 

at  45°- 

o.oo 

o 

•  OO 

O 

•340 

O 

.667 

0 

.02 

1.70 

0-340 

0.666 

O-O2 

I 

.17 

O 

339 

0 

.663 

O 

•05 

8.5I 

o-339 

0.663 

O.O5 

2 

•93 

0 

•335 

0 

•654 

O 

•  2O 

17  .02 

0-333 

0.647 

O-2O 

II 

.70 

o 

336 

0 

.617 

O 

•50 

42-54 

0.319 

0.613 

0.50 

29 

•25 

o 

.282 

0 

•546 

I 

.00 

85.09 

0.294 

1.  00 

58 

•50 

o 

•449 

59 


BENZOIC    AOID 


SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS   SOLUTIONS  OF  SODIUM 
ACETATE,  FORMATE,  BUTYRATE,  AND  SALICYLATE. 

(Noyes  and  Chapin  — Z.  physik.  Chem.  27,  443,  '98;  Philip  —  J.  Ch.  Soc.  87,  992,  '05.) 


Grams 

Gram; 

3  CeH5COOH 

per  Liter  of  S< 

>lution  in: 

Sodium 
Salt  per 

CHgCOONa. 

HCOONa. 

CaHyCOONa.  Qj^OH.COONa. 

Liter. 

At  25°. 

At  26.  46. 

At  25°. 

At  26.4°. 

At  26.4°. 

At  26.4°. 

O 

3-4i 

3-53 

3-41 

3-53 

3-53 

3-53 

I 

4-65 

4-75 

4-25 

4-35 

4-50 

3-62 

2 

5-7o 

5-85 

4-75 

4-85 

5-40 

3  •  7o 

3 

6.70 

6.90 

5-20 

5-30 

6.15 

3  •  80 

4 

7.60 

7-85 

5-6o 

5-70 

6.90 

3-87 

6 

8.40 

4.00 

8 

.  .  . 

.  .  . 

.  .  . 

.  .  . 

.  .  . 

4.10 

Sodium  Salt 

CH3COONa. 

HCOONa. 

C3H7COONa.  CeH^OH.COONa 

per  Liter. 

At  25°. 

At  26.4°. 

At  25°. 

At  26.4°'. 

At  26.4°.             At  26.4°. 

O 

.00 

O 

.0279 

O 

.0289 

0.0279 

0.0289 

O 

.0289 

0.0289 

O 

.01 

O 

.0362 

0 

.0370 

0.0330 

0-0336 

0.0376 

0-0300 

O 

.02 

O 

.0440 

0 

.0448 

0.0364 

0.0372 

O 

•°455 

0.0312 

0 

•03 

O 

.0508 

0 

.0518 

0.0392 

0.0398 

o 

•0525 

0.0321 

O 

.04 

O 

.0572 

0 

.0586 

O.O4l6 

0-0423 

0 

.0596 

0.0328 

O 

.06 

o  .  0460 

o  .  0466 

0.0342 

SOLUBILITY  OF  BENZOIC  ACID  IN  ABSOLUTE  ALCOHOLS. 

(Tiirofeiew  —  Compt.  rend.  112,  1137,  '91;  at  15°,  Bourgoin  —  Ann.  chim.  phys.,  [5]  13,  406,  '78.) 

In  Ethyl  Alcohol. 


In  Methyl  Alcohol. 


G.  C6H5COOH 

per  loo  Gms. 


G.  C6H5COOH 

per  100  Gms. 


In  Propyl  Alcohol. 

G.  CeHeCOOH 
per  100  Gms. 


3 
15 

21 


CH3OH. 
50.l6 


Solution. 

33-39 


69.29        40.93 


C2H5OH. 
4O.l6 
46.70 
54-09 


Solution. 
28.65 
31.80 

35  ^o 


C3Jti7OH. 
29.88 


Solution. 
23.00 


40 .64  28 . 90 


SOLUBILITY  OF  BENZOIC  ACID  IN  90%  ALCOHOL,  IN  ETHER  AND  IN 

CHLOROFORM. 

(Bourgoin.) 


Solvent. 


Gms.  C6H5COOH  per  TOO  Grams. 


90%  Alcohol 

Ether 

Chloroform 


15 
15 
25 


Solvent. 
41  .62 

3r-35 
14.30 


Solution. 

29-39 
23.86 

12  .50 


SOLUBILITY  OF  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  DEXTROSE. 


Normality  of 
Aq.  Dextrose. 

Gms.  CeHi2( 
per  Liter. 

0.02 

3-67 

O.O5 
O.2O4 

0-533 
1.  068 

9-OO 

36.73 
96.15 

192.30 

(Hoffman  and  Langbeck.) 
Dissolved  CeHsCOOH  at  25°. 


Mol.  Cone. 

Weight 
Per  Cent. 

5-0322.IO"4 

o-34 

5-0403    " 

o-34 

5-0303    " 

o-34 

5-032I    ' 

o-34 

5-0443  " 

0-341 

Dissolved  CeHsCOOH  at  4<°. 


Mol.  Cone. 

Weight  " 
Per  Cent. 

9.  9088.  io~  4 

0.674 

9.9328    " 

0.669 

9.9323    " 

0.669 

IO-OIOI    *' 

0-674 

10-0,369  " 

0.676 

BENZOIO    AOID  60 

SOLUBILITY  OP  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  UREA  AND 

OF  THIO  UREA. 

(Hoffman  and  Langbeck.) 

Normality  Cms.  CaHsCOOH  Dissolved  at  25°. 

of  Solution.  per  Liter.  Mol.  Cone.      Wt.  per  cent. 

In  Aqueous  Urea  o.io        6.01  CO(NH2)2      5-i876.io~4     0.350 

In  Aqueous  Thio  Urea    0.20      15.23  CS(NH2)2       5-4994    "         0.372 

Amido  BENZOIO    ACIDS     C6H4.NH2.COOH  (m). 

SOLUBILITY  IN  WATER  AND  IN  OTHER  SOLVENTS. 

(de  Coninck  —  Compt.  rend.  116,  758,  "93.) 

In  Water.  In  Organic  Solvents. 

Gms.  Gms. 

t°.    CflH4.NH2.COOH(m)  Solvent.  t°.       CeH4.NH2.COOH(m) 

per  100  cc.  H2O.  per  100  cc.  Solvent. 

o  0.43  Ethyl  Alcohol  (95%)  12.5  2.92 

10  0.52  Methyl  Alcohol  (pure)  10.5  4.05 

20  0.67  Acetone  11.3  6.22 

30  0.87  Methyl  Iodide  10.0  0.04 

40  1.15  Ethyl  Iodide  o.o  0.02 

50  1.50  Chloroform  12.0  0.07 

60  2.15  Bromoform  8.0  trace 

7o  3-iS 

SOLUBILITY  OF   THE  THREE  ISOMERIC  AMIDO  NITRO  BENZOIC  ACIDS. 
In  Ether.  In  Ethyl  Alcohol  (90%). 

Gms.  C6H3.NO3.NH2.COOH  Gms.  QjH3NO3.NH2.COOH 

.  o  per  100  cc.  Ether.  f  0  per  100  cc.  Alcohol. 


Ortho.  Meta.        Para.  Ortho.         Meta.          Para. 

2.7  10.84  1.70    6.41        3  8.13       1.79        8.4 

5.8  16.05  (6.8°)     1.81     8.21        9.6      10.70      2.20      11.3 

SOLUBILITY  IN  WATER  OF  THE  THREE  ISOMERIC: 

(Vaubel  — J.  pr.  Chem.  [2]  52,  72,  '95-) 

Amido  Benzo  Sulphonic  Acids.  Amido  Phenols. 

G.  C8H4.NH2.SO2H  per  100  g.  Aq.  Sol.  o    G.  C6H4(OH).NH2  per  100  g.  Aq.  Sol. 

Ortho.  Meta.  Para.  Ortho.  Meta.  Para. 

7        i. 06        1.276        0.592  (6°)        o         1.7      2.6(20°)        i.i 

Brom,  Chlor,  and  lodo  BENZOIG    ACIDS. 

SOLUBILITY  IN  WATER  AT  25°. 

(Paul  —  Z.    hysik.  Chem.  14,  in,  '94;  Lowenherz  —  Ibid.  25,  401,  '98;  Vaubel.) 

Per  1000  cc.  Aqueous  Solution. 

Compound.  Formula.  / « * 

Grams.       Gram  Mol. 

Brom  benzoic  acid.  CeH4Br.COOH  (ortho).  1-856  0.00924 

Brom  benzoic  acid.  CcH4Br.COOH  (meta).  0.402  0-00200 

Brom  benzoic  acid.  C6H4Br.COOH  (para).  0.056  0-00028 

Chlor  benzoic  acid.  C6H4C1.COOH  (ortho).  2.087  0.01333 

lodo  benzoic  acid.  CflH4I.COOH     (ortho).  0.95 

lodo  benzoic  acid.  CeH4I.COOH    (meta).  0.12 


6i 


BENZOIO   ACIDS 


SOLUBILITY  OF  ORTHO  HYDROXY  BENZOIC  ACID  (SALICYLIC  ACID),  META 
HYDROXY  BENZOIC  ACID,  AND  PARA  HYDROXY  BENZOIC  ACID  (ANISIC 
ACID)  IN  WATER,  BENZENE,  ETC.  (See  also  pp.  38  and  274.) 

(Walker  and  Wood  — J.  Ch.  Soc.  73,  622,  '98;  Vaubel  — J.  pr.  Chem.  [2]  52,  73,  '95.) 

ioo  gms.  aq.  solution  contain  0.225  gm.  C6H4.OH.COOH  (o)  at 
15°  (Vaubel). 

ioo  gms.  aq.  solution  contains  0.794  gm.  C6H4.OH.COOH  (p)  at 
15°  (Vaubel). 


Gms.  C  H4.OH.COOH 
to^                    per  ioo  Gms.  H2O. 

10 

Meta. 

o-55 

Para. 
0.25 

20 

25 
30 

35 

0.90 
i.  08 

i-34 
i  .64 

0.50 
0.65 

0.81 

I  -01 

40 

2  .IO 

1.24 

50 
60 

3.10 

2.12 

80 

.  .  . 

In  Acetone. 

G.  CeH4.OH.COOH 

per  loo^cc.  Sol. 

Meta.  Para! 

26.O  22-7 


Gms.  C6H4.OH.COOH 

per  ioo  Gms.CeHa. 

Meta. 

Para. 
O.OOlS 

O.OO8 

0.0027 

0-010 

0.0035 

0-012 
O.OI5 
0.017 
0.028 

o  -  0045 
o  .  0060 

0.0082 
0.0162 

0-047 

O.O28 
O.O66 

In  Ether. 

G.  QH4.OH.COOH 

per  ioo  cc.  Sol. 

Meta.  Para'. 

9-73        9-43 


Methyl   BENZOIO    ACIDS     C6H4COOH.CH3.     o,  m,  and  p. 
SOLUBILITY  IN  WATER. 

(Vaubel.) 
Gms.  CaHiCOOH.CHa  per  1000  Gms.  Sat.  Solution. 


Ortho. 

1.18 


Meta. 
0.98 


Para. 
0-35 


Nitro  BENZOIO    ACIDS     C6H4.NO2.COOH.     o,  m,  and  p. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 


(de  Coninck  —  Compt.  rend.  118,  471 
and  Gold 


tfor  solubility  in  H2O,  see  also  Paul,  Vaubel,  Lowenherz, 
—  Z.  physik.  Chem.  25,  95,  '96.) 

Gms.  C6H4.NO2.COOH  per  ioo  cc.  Solvent. 


ouiveui. 

v    • 

Ortho. 

Meta. 

Para. 

Water 

20 

0.682  (0.654G.) 

0.3IS 

0.039 

Water 

25 

0-743-0-779 

0.341 

O.O28 

Water 

30 

0.922 

.  .  . 

Methyl  Alcohol 

10 

42.72 

47-34 

9.6 

Ethyl  Alcohol 

10 

28.2 

33-i(ii.70) 

0-9 

Ethyl       "(33Vol.%) 

15 

0.64(11.8°) 

0.52 

0-055 

Acetone 

10 

41-5 

4i-5 

4-54 

Benzene 

10 

0.294 

o-795 

0.017(12.5°) 

Carbon  Bi-Sulphide 

10 

O-OI2 

0-10(8.5°) 

0.007 

Chloroform 

10 

0.455  C11-0) 

5  -678 

0.066 

Ethei 

10 

21.58 

25-I75 

2  .26 

Ligroin 

10 

trace 

0-013 

0-00 

BENZOIO    ACIDS  62 

SOLUBILITY  OF  PARA  NITRO  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS 
OF  ANILIN  AND  OF  PARA  TOLUIDIN  AT  25°. 

(Lowenherz —  Z.  physik.  Chem.  25,  395,  '98.) 

In  Anilin.  In  ^-Toluidin. 

G.  Mols.  per  Liter.  Gms.  per  Liter.  G.  Mols.  per  Liter.  Gms.  per  Liter. 

' 


aHcNHa 

C6H4.N02. 
COOH. 

C6H5NH2 

•    C04OH2' 

cggra-  »* 

C6H4NH2- 
CH3. 

C«H4N02. 
COOH. 

O-O 

0-00164 

0-0 

0 

.274 

o 

.0 

0 

.00164 

O 

.0 

0-274 

O-OI 

0.00841 

0.91 

I 

.406 

o 

.01 

0 

•  OIOO 

I 

.071 

I  .671 

O-O2 

0.01379 

1.82 

2 

•304 

0 

.02 

0 

.0174 

2 

.142 

2  .902 

O.O4 

0.02172 

3-64 

3 

.629 

o 

•03 

0 

.0245 

3 

.213 

4-097 

0.08 

0.0347 

7.29 

5 

.798 

SOLUBILITY  OF  ORTHO  NITRO  BENZOIC  ACID  IN  AQUEOUS  SOLU- 
TIONS OF  SODIUM  BUTYRATE,  ACETATE,  FORMATE,  AND 
SALICYLATE  AT  26.4°. 

(Philip  —  J.  Chem.  Soc.  87,  992,  '05.) 

.  Mols.         ,. 
Original  results  in  terms  of •  per  liter. 


Gms.  Na  Salt 

Urns.  Ur 

tno  U8ii4UUUJl.. 

NU2  per  .Liter  o 

t  solution  in: 

per  Liter. 

C3H7COONa. 

CH3COONa. 

HCOONa. 

C6H4.OH.COONa. 

0 

7-85 

7-85 

7-85 

7-85 

o-5 

8-35 

8.50 

8.60 

8-35 

I.O 

8.90 

9-15 

9-50 

8.70 

2 

IO-O 

I0.8o 

"-5 

9-4 

3 

II  .2 

12-55 

13  .5 

II  .0 

4 

12-4 

14-5 

15-6 

JI-5 

6 

15.2 

SOLUBILITY  OF  ORTHO  NITRO  BENZOIC  ACID  IN  AQUEOUS  SOLUTIONS 
OF  DEXTROSE,  SODIUM  CHLORIDE,  AND  OF   SODIUM    NITRATE. 

Original  results  in  molecular  quantities. 

(Hoffman  and  Langbeck  —  Z.  physik.  Chem.  51,  412,  '05.) 
In  Dextrose.  In  NaCl.  In  NaNO3. 


G.  C6H12Oa 
per  loo  cc. 
Solution. 

o.o 

0.36 
1.  80 

9-50 
2O.OO 

G.(o)C6H4 
per  100 

N02.COOH 

g.  Solvent. 

G.  NaCl. 
per  100  cc 
Solution. 

O.II7 
0.195 

0.585 
2.425 

5-80 

G.(o)C6H4N02.COO 
per  100  g.  Solvent. 

H  G.NaNO3 
per  100  cc. 
Solution. 

O.I7O 
0.284 
0-851 
4-255 
8.510 

v 

G.(o)C6H4N02.COOH 
per  TOO  g.  Solvent. 

At  25°. 
0.736 
0.736 
0.732 
O.722 
0.703 

At 
I  . 
I  . 
I  . 
I  . 
I  . 

35°. 
063 
064 

061 

051 
030 

At  25°. 

o-743 
0.746 

0.749 
0.688 

o-597 

At  35°. 
I  .072 

1-075 
I  .O7O 
0-967 
0.831 

At  25°. 
0.746 

o-754 
0.767 
0.774 
0.748 

At  356- 
1.074 
I.OSO 
I  .096 
1.097 

1.047 

BENZOIO    SULPHINIDE    (Saccharine)     C6H4<^J2>NH. 

100  parts  water  dissolve  0.4  part  at  25°  and  4.17  parts  at  100°. 
100  parts  alcohol  dissolve  4  parts  at  25°  (U.  S.  P.). 


BENZOPHENONE 


BENZOPHENONE  (C6H5)2CO. 

SOLUBILITY  IN  AQUEOUS  ALCOHOL  AND  IN  OTHER  SOLVENTS. 

(Derrien  —  Compt.  rend.  130,  722,  'oo;  Bell  —  J.  Physic.  Chem.  9,  550,  '05.) 

In  Aqueous  Alcohol  at  40°. 

(Bell.) 

Wt.  %      Gms.  (C6H5)2CO 
Alcohol        P61"  I0°  Gms. 


>olven 

t-  Solvent. 

Solution. 

40 

2 

I.Q 

45 

5 

4-8 

50 

8 

8-3 

55 

ii 

9.9 

60 

16 

13-8 

65 

28 

22.6 

Wt.% 

Gms.  (C6H5)2CO 

Alcohol 

per  100  Gms. 

in  Solvent. 

Solvent.      Solution. 

67.5 

39        28.1 

70 

56        35-9 

71 

67        39.2 

72 

90        47.4 

72-5 

105        51.2 

73 

156        61.0 

In  Aqueous  Alcohol  and  other  Solvents. 

(Derrien.) 


Solvent. 

97%  Ethyl  Alcohol  17 

85  cc.  97%  Alcohol  +  iscc.  H2O  " 
80 "  "      +  20  " 

75"  "       +26" 

Methyl  Alcohol  (pure)  9.8 

15.0 

Acetic  Ether  (pure)  9.6 

Carbon  B  isulphide  1 6 .  i 


Gms. 
(C6H5)2CO 
per  100  g. 
Solvent. 


Solvent. 


13-5 
3-8 

2  .2 

*-3 

II  .O 

14-3 
19.2 
66.6 


Benzene 

Xylene 

Nitro  Benzene 

Chloroform  (com.) 

Bromoform 

Toluene 

Ligroine 


15-8 
16.5 

!7-3 
17.2 
14.6 


Gms. 

(C6H5)2CO 
per 

100  g. 

Solvent. 
76.9 
38-4 
58.8 

55-5 

33-3 

55-5 

6.7 


BERYLLIUM  HYDROXIDE  Be(OH)2  (See  also  Glucinium,  page  140). 
SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  HYDROXIDE. 

(Rubenbauer  —  Z.  anorg.  Chem.  30   334,  '02.) 

Moist  Be(OH)2  used,  solutions  shaken  5  hours,  temperature  prob- 
ably about  20°. 

Gms.  per  100  cc.  Solution. 
'NaOH.  Be(OH)2.' 


Per  20  cc.  Solution. 

Molecular 
Dilution 

Gms.  Na. 

Gms.  Be. 

of  the 

NaOH. 

Q-3358 

0.0358 

1.37 

0-6716 

0.0882 

0.68 

0.8725 

0-II75 

o-53 

I-7346 

0-2847 

0.27 

2.917 
5.840 

18.310 


BERYLLIUM    SULPHATE     BeSO,. 

SOLUBILITY  IN  WATER. 

(Levi,  Malvano  —  Z.  anorg.  Chem.  48,  446,  '06.) 


0.850 
2.094 

2.789 
6.760 


31 

50 
72 

77 
30 
40 
68 
85 

Mols.  H2O 
per  i  Mol. 
BeS04. 

II.  18 
9.62 
.2          7.79 

•4      7-!3 
13-33 
12.49 
9.42 
7-65 

Gms.  BeSO4  per 

100  Gms. 

Solid 
Phase. 

BeS04.6H2O 
BeSO4.4H2O 

95- 
107. 
in 
80 
91. 

119 

Mols.  H2O 
per  i  Mol. 
BeS04. 

4      6.44 
2       5.06 

4-55 

6.89 
4     5-97 
4-93 
3-91 

Gms.  BeSO4  per 
100  Gms. 

Solid 
Phase. 

BeSO4.4H  O 
BeSO4.aH,O 

Water. 

60-67 

74-94 
81.87 
43-78 
46.74 
61.95 
76.30 

Solution  . 
34-32 

37-77 
42.85 
45.01 
3°-45 

38.27 
43.28 

Water. 
90.63 

II5-3 
128.3 
84.76 

97-77 
118.4 

149-3 

Solution. 

47-55 
53.58 
56.19 

45-87 
49.42 

54-21 
59-88 

BISMUTH 


64 


BISMUTH     Bi. 

MUTUAL  SOLUBILITY  OF  BISMUTH  AND  ZINC. 

(Spring  and  Romanoff  —  Z.  anorg.  Chem.  13,  34,  '96.) 


0             Upper  Layer.  Lower  Layer. 

'%Bi.        %Zn."  %Bi.      %Zn. 

266    86    14 

419  3    97 

475    84    16  5    95 


0  Upper  Layer.          Lower  Layer. 

%Bi.       %Zn.        %Bi.       %Zn. 
584  80  20  10  QO 

650  77  23  15  85 
750  70  30  27  73 
810-820  (crit.  temp.) 


BISMUTH    CHLORIDE     BiCl3. 

100  grains  absolute  acetone  dissolve  17.9  grams  BiCl3  at  18°. 

(Naumann  —  Ber.  37,  4332,  1004.) 

BISMUTH    IODIDE     BiI3. 

100  grams  absolute  alcohol  dissolve  3.5  grams  BiI3  at  20°. 

(Gott  and  Muir  —  J.  Chem.  Soc.  57,  138,  '90.) 

ioo  grams  methylene  iodide  CH2I2  dissolve  0.15  gram  BiI3  at  12°. 

(Retgers  —  Z.  anorg.  Chem.  3,  343,  '93.) 

BISMUTH    NITRATE    Bi(NO3)3.sH2O. 

ioo  grams  acetone  dissolve  48.66  grams  Bi(NO3)3.5H2O  at  o°,  and 
41.7  grams  at  19°. 

(von  Laszczynski  —  Ber.  27,  2285,  '94.) 


BISMUTH    OXIDE    Bi2O3. 
SOLUBILITY  OF  BISMUTH  OXIDE  IN  AQUEOUS  NITRIC  ACID  AT  20°. 

(Rutten  and  van  Bemmelen  —  Z.  anorg.  Chem.  30,  386,  '02.) 


Present  in  Shaker 
Flask. 

Gms.  per  ioo  Gms. 
Solution. 

Mols.  per  ioo  Mols.  H2O. 

Solid 

Per  i  part  Bi2O3. 
3N2O5.ioH2O. 

Bi203 

N205 

Bi203 

N206  Ra!i°BcJ>2°3 
:  JN  2<->5. 

Phase. 

24.4  parts  H2O 
3.2partsH2O 

0.321 

0.963 
7.17 

o  126 
2.844 

I 

.61 

.82 

i 

12 

4 

.8 
.8 

Bi2O3.N206.2H2O 

Dilute  HNO3 
Dilute  HNO3 

l8'37 
3148 

15-9 
23-7 

10.50 
27.2 

$ 
83 

•65 

.8 

i 

3 
3 

.6 

.0) 

Bi2O8N205.HjO 

Dilute  HNO3  = 
6.13%  N205 

32-93 

24.83 

97 

•97 

i 

3 

.2 

(Bi2OvN205.H2Oand 
Bi203.3N2O6.ioH20 

6.816%  N205 

32.67 

24.70 

29.70 

96.57 

i 

3 

•21 

24.0%  N2O6 
51.0%  N2O6 

24.16 
11.66 

28.25 
46.62 

19.65 
10.81 

98 
186 

.76 
•23 

i 
i 

r 

.0 

.2 

>-Bi2O3.3N2O5.ioH2O 

70.0%  N2O6 

20.76 

53-75 

33-51 

355 

.87 

i 

io.6j 

Anyhdrous  HNO 
Bi2O3+      " 

27.85 
38.56 

4.05 

51.02 
68.28 
74.90 

51.0 

14-35 
7-45 

403.0 
492.0 
592.9 

i 
i 
I 

7-9 
34-3 

79-5  J 

Bi203.3N205.ioH2O 
Bi203.3N205.3H20 

Bia08.3Na06.3HaO 

and 

Results  are  also  given  for  9°,  30°,  and  65°. 


65  BORIC  ACID 

BORIC  ACID     (Ortho)    H3BO3. 

SOLUBILITY  IN  WATER. 

(Ditte  —  Compt.  rend.  85,  1069,  77;  Herz  and  Knoch  —  Z.  anorg.  Chem.  41,  319,  '04.) 


Gms.  H3BO3  per 
f^            ioo  Gms. 

Gms.  B2O3 
per  ioo  Gms.              t°. 

Gms.  HsBO3  per 
ioo  Gms. 

Gms.  EyO3 
per  ioo  Gms. 

\Y 

ater. 

Solution. 

H20. 

'Water. 

Solution. 

O 

I 

•95 

I 

.91 

I 

.1 

40 

7-0 

6-54 

3 

•95 

10 

2 

.70 

2 

•63 

I 

•5 

5o 

8.8 

8.09 

5 

.08 

20 

4 

.0 

3 

•85 

2 

•25 

60 

II  .0 

9.91 

6 

.2 

25 

4 

•7 

4 

•49 

2 

•65 

80 

16.8 

14-38 

9 

•5 

30 

5 

•4 

5 

.12 

3 

•05 

IOO 

27-5 

2i-57 

15 

•52 

The  above  results  of  Ditte  are  probably  low. 

Herz  and  Knoch  find  for  13°,  3.845  grams  H3BO3  per  100  cc.  solution, 
for  20°,  4-909,  25°,  5.593,  and  26°,  5.637. 

Bogdan  finds  5.753  grams  H3BO3  per  100  grams  H2O  at  25°. 


SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC, 
SULPHURIC,  AND  NITRIC  ACIDS  AT  26°. 

(Herz  —  Z.  anorg.  Chem.  33,  355,  34,  205,  '03.) 

Normality  of      Normality  of 
the  H2S04,  HC1       Dissolved 
or  HN03.  B(OH)3. 

o  0.91 

0-5  0.78 

i .o  0.71 

2.0  0.58 

3.0  0-49 

4-0  0.41 

5-o  0.35 

6.0  0.26 

The  determinations  given  in  the  original  tables  in  terms  of  normal 
solutions  when  plotted  together  lay  close  to  an  average  curve  drawn 
through  them.  The  figures  in  the  tables  here  shown  were  read  (and 
calculated)  from  the  average  curve. 


SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ELECTROLYTES 


Gms.  Strong  Acid         Gms.  B(OH)3  per  ioo  cc 

.  Solution. 

Solution. 

In  HC1. 

In  H2SO4. 

In  HNO3. 

0 

5-64 

5-64 

5.64 

5 

4.0 

4-25 

4-5° 

10 

3-2 

3-6 

3-9 

I5 

2-45 

3-o 

3-35 

20 

1.8 

2-5 

2.9 

25 

2.0 

2-55 

30 

!-55 

2  .1 

35 

J-75 

AT    25 


(Bogdan  —  Ann.  Scient.  Univ.  Jassy,  2,  47,  'o2-'o3.) 


Gms.  Electro- 

Grams  H3BO3  per  100  Gms.  H2O  in  Aq.  Solutions  of: 

lytc  per  100 
Gms.  H2O. 

NaCl. 

KCl. 

NaNO3. 

KNO3. 

Na2S04. 

K2S04. 

O 

5-75 

5-75 

5-75 

5-75 

5-75 

5-75 

10 

5-75 

5.80 

5-78 

5.81 

5.88 

5-92 

20 

5-74 

5.86 

5.81 

5-88 

6.00 

6.10 

40 

5-72 

5-98 

5-87 

6.04 

6-33 

6.50 

60 

5-72 

6.12 

5-95 

6.  20 

6.70 

6.92 

80 

5-71 

6.29 

6.  02 

6.37 

7.10 

7.40 

Interpolated  from  the  original. 

100  parts  alcohol  dissolve  6.5  parts  H3BO3  at  25°  and  23  parts  at 
b.  pt.  (U.  S.  P.). 


BORIO    ACID 


66 


SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  UREA,  ACE- 
TONE, AND  OF  PROPYL  ALCOHOL  AT  25°. 

(Bogdan.) 


Grams  of 

CO(NH2)2,(CH3)2CO 

or  of  CaHyOH  per 

100  Cms.  H2O. 

O 
10 
20 

40 

60 


Cms.  H3BO3  per  100  g.  H2O  in  Aq. 
Solutions  of: 


CO(NH2)2 

(CH3)2CO. 

CsH7OH. 

5-75 

5-75 

5-75 

5-84 

S-84 

5-80 

5-93 

5-93 

5-85 

6.13 

6.12 

5-94 

6-31 

6.29 

6.03 

SOLUBILITY  OF  BORIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  : 


Acetic  Acid  at  26°. 

(Herz  —  Z.  anorg.  Chem.  34,  205,  '03.) 
Normality  of  Solutions.        Cms.  per  100  cc.  Solution. 


CW3COOH. 

B(OH)3. 

CH3COOH. 

B(OH)3. 

O 

0.91 

0 

5.64 

I 

0.82 

5 

4-7 

2 

0.65 

10 

4.2 

4 

0.42 

20 

3-° 

6 

0.25 

30 

2.O 

Acetone  at  20°. 

(Herz  and  Knoch  —  Ibid.  41,  319,  '04.) 


cc.  Acetone 
per  100  cc. 
Solvent. 

B(OH)3  per 

TOO  cc.  Solutioi 

Millimols. 

Grams. 

0 

79-15 

4.91 

20 

81.71 

5-07 

30 

83-35 

5-17 

40 

82.72 

5-*3 

50 

81.62 

5.06 

60 

76.40 

4-74 

70 

67.62 

4.19 

80 

55-05 

3-4i 

100 

8.06 

0.50 

Pure  Glycerine  (Sp.Gr.  =1.260 
at  15.5°). 

(Hooper  —  Pharm.  J.  Trans.  [3]  13,  258,  '82.) 


SOLUBILITY  OF  BORIC  ACID  IN: 

Aq.    Solutions  of  Glycerine 
at  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  45,  268,  '05.) 


Gms.  B2O3 
t  o     3H2O  per 

100   CC. 

Glycerine 

•-   Gms.  B(OH)3  per  100 
Gms. 

Wt.  %          Millimols 
Glycerine   B(OH)3  per 
in  Solvent.    100  cc.  Sol. 

Sp.  Gr. 
25° 

Gms.  B(OH)a 
per  100 

Glycerine.  Solution. 

a<4°' 

cc.  Solution 

Gms.So- 
*    lution. 

O 

20 

I5-87 

!3 

•17 

O 

90.1 

I    .OI7 

5 

•59 

5-50 

IO 

24 

19.04 

16 

.00 

7 

•15 

90.1 

1.038 

5 

•59 

5-38 

2O 

28 

22  .22 

18 

.21 

20 

•44 

90.6 

1.063 

5 

.62 

5.28 

30 

33 

26.19 

20 

•75 

31 

•55 

92.9 

I    .090 

5 

.76 

5-29 

40 

38 

30.16 

23 

•17 

40 

•95 

97-0 

I.II3 

6 

.02 

5  -41 

50 

44 

34-92 

25 

•95 

48 

•7 

103.0 

I-I33 

6 

•39 

5-64 

60 

50 

39-68 

28 

.41 

69 

.2 

140.2 

1.187 

8 

.69 

7-32 

70 

56 

44-65 

30 

•72 

100 

•  O 

390-3 

1.272 

24 

.20 

19.02 

80 

61 

48.41 

32 

.61 

• 

90 

67 

53-18 

34 

.70 

100 

72 

57-14 

36 

•36 

67  BORIC    ACID 

DISTRIBUTION  OF  BORIC  ACID  BETWEEN  WATER  AND  AMYL  ALCOHOL 

AT    25°. 
(Fox  —  Z.  anorg.  Chem.  35,  130,  '03.) 

Millimols  B(OH)3  in       Cms.  B(OH)3  in  100  cc.    Millimols  B(OH)3  in       Cms.  B(OH)3  in  100  cc 


'Aq. 

Alcoholic 

Aq. 

Alcoholic 

Aq. 

Alcoholic 

Aq. 

Alcoholic 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

265.8 

76.6 

I 

.648 

0 

•475 

87 

•9 

33 

.2 

Q-545 

O.206 

196.5 

59-5 

I 

.219 

o 

369 

75 

.2 

22 

•7 

0.466 

o.  141 

159.6 

47-5 

O 

.990 

o 

,294 

64 

.6 

J9 

.76 

0.400 

0.123 

I26.O 

37-i 

o 

.78l 

0 

,230 

BORIC    ACID    (Tetra)    H2B4O7. 

100  grams  water  dissolve  2.69  grams  H2B4O7  at  15°,  Sp.  Gr.  =  1.015. 

(Gerlach  —  Z.  anal.  Chem.  28,  473,  '89.) 


BORON    TRI-FLUORIDE    BF3. 

i  cc.  H2O   absorbs    1.057  cc-  BF3  at  o°  and   762   mm.,  i  cc.  cone. 
H2SO4  (Sp.  Gr.  1.85)  absorbs  50  cc.  BF3. 


BROMINE    Br. 

SOLUBILITY  IN  WATER. 

(Winkler  —  Chem.  Ztg.  23,  687,  '99;  Roozeboom  —  Rec.  trav.  chim.  3,  29,  59,  73,  84,  '84;  Dancer  — 
J.  Chem.  Soc.  15,  477,  '62;  at  15°,  Dietze  —  Pharm.  Ztg.  43,  200,  '98.) 

Grams  Bromine  per  100  Grams.  "Absorption 

Coefficient."*  Solubility.    * 

a.  q. 

60.5  43-1 

45.8  32.4 

35-1  24.8 

27.0  19.0 

21-3  14.8 

17.0  II.7 

I3.8  9.4 

9.4  6.2 

6.5  4-0 

4.9  2.8 

3-0  I.I 

*  For  "  Absorption  Coefficient "  a  and  "Solubility"  q,  of  Bromine  Vapor  in  water,  see  Acetylene, 
page  9- 


t°. 

t  — 

Water. 

Solution  . 

(W.) 

(R.  D.  &  D.) 

(W.) 

(R.  D.  &  D.) 

0 

4.17 

4-22 

3-98 

4-05 

5 

3-92 

3-7 

3-77 

3-57 

10 

3-74 

3-4 

3.61 

3-29 

15 

3-65 

3-25 

3-52 

3-!5 

20 

3-58 

3.20 

3-46 

3.10 

25 

3-48 

3-17 

3-36 

3-o7 

30 

3-44 

3-!3 

3-32 

3-03 

40 

3-45 

3-33 

50 

3-52 

3-40 

60 

80 

.  .  . 

.  .  . 

BROMINE 


68 


SOLUBILITY  OF  BROMINE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM  Sui/- 
PHATE,  SODIUM  SULPHATE,  AND  OF  SODIUM  NITRATE  AT  25°. 

(Jakowkin  — Z.  physik.  Chem.  20,  38,  '96.) 


Normality  of            Gms.  per  Liter. 

n    I*.    Q-1-.  *:,-._.                                           *^  *- 

In  Na2SO4 
Gms.  per  Liter. 

In  NaNO8 
Gms.  per  Liter. 

KabO4. 

Br. 

Na2S04. 

Br. 

NaN03. 

Br. 

i                 9I.l8 

25.14 

63.55 

25.07 

85.09 

28.80 

i            45-59 

29.44 

31*77 

29.20 

42-54 

31-35 

i           22.79 

31.46 

15.88 

3*  -33 

21.27 

32.62 

i           n-39 

32.70 

7-94 

32-94 

10.63 

33-33 

iV            5-69 

33  -I0 

3-97 

32.26 

5-31 

33-74 

SOLUBILITY  OF  BROMIN£  IN  NORMAL  AQUEOUS  SALT  SOLUTIONS 

AT  25°. 

(McLauchlan  —  Z.  physik.  Chem.  44,  617,  '03.) 


Gms. 

Normality 

Gms. 

Gms. 

Normality 

Gms. 

Salt. 

Salt 

per 

of 

Dis- 

Br.  per 

Salt. 

Salt 

per 

of 

Dis- 

Br.  per 

Liter. 

solved  Br. 

Liter. 

Liter. 

solved  Br. 

Liter 

Water 

O  . 

O 

0. 

424 

33-95 

NH4NO3 

80. 

II 

0. 

688 

55-15 

Na2SO4 

63- 

55 

0. 

286 

23-9 

NaCl 

58- 

50 

O  . 

701 

55-90 

K2S04 

91. 

18 

0. 

3IO 

24.8 

KC1 

74- 

60 

o. 

718 

57-40 

(NH4)2S04 

70. 

04 

o. 

971 

77-7 

NH4C1 

53- 

52 

I  . 

028 

82.2 

NaNO3 

85- 

09 

O. 

3495 

28.0 

CH3COONH4 

77- 

09 

4- 

26 

340-5 

KN03 

101. 

19 

0. 

362 

28=95 

H2S04* 

49. 

°3 

0. 

366 

29.26 

*  Wildeman. 


SOLUBILITY  OF  BROMINE  IN  AQUEOUS  POTASSIUM  BROMIDE  SOLUTIONS. 

(Worley  —  J.  Chem.  Soc.  87,  1107,  '05;  see  also  Wildeman  —  Z.  physik.  Chem.  II,  421,  '93.) 


Gram  Mols.  KBr    Gms.  KBr 

Br.  per  Liter  Dissolved  at  26.5°. 

Br.  per  Liter  Djssolved  at  18.5°. 

per  Liter. 

per  Liter. 

G.  Mols. 

Grams. 

G.  Mols. 

Grams. 

O-OO 

o.oo 

0.4282 

34-23 

o  .  4448 

35-56 

O-O2 

2.18 

0-4671 

37-35 

0.4823 

38.56 

O.O4 

4-38 

0.5IOI 

40.79 

0.5243 

41.91 

0-06 

6-55 

0-5530 

44.21 

0.5668 

45  -31 

0.08 

8.76 

0.5920 

47-33 

o  .  6059 

48.44 

o.io 

10.91 

0.6488 

5I-87 

0-6533 

52-23 

O.2O 

21.82 

0.8591 

68.69 

0-8718 

69.69 

O.4O 

43.82 

1.2704 

101.60 

I.3I24 

104  .  90 

0.6o 

65.46 

1.6717 

I33-70 

I.77I2 

141  .60 

0.80 

87.64 

2.1029 

168.10 

2.2354 

178.70 

0.90 

98.19 

2-3349 

186.20 

2.4851 

198.70 

ioo  grams  saturated  solution  of  Bromine  in  Carbon  Bisulphide  con- 
tain 45.4  grams  Br  at  —  95°,  39.0  grams  at  —  110.5°,  and  36-9  grams 
at  -  116°. 

(Arctowski  —  Z.  anorg.  Chem.  n,  274,  *95-'96.) 


BROMINE 


DISTRIBUTION  OF  BROMINE  AT  25°  BETWEEN  WATER  AND: 

(Jakowkin  — Z.  physik.  Chem.  18,  588,  '95.) 


Carbon  Bisulphide. 


Bromoform. 


Carbon  Tetra  Chloride. 


Cms.  Br. 

per  Liter  of: 

Cms.  Br. 

per  Liter  of: 

Gms.  Br. 

per  Liter  of: 

Aq.  Layer. 

CS2  Layer. 

Aq.  Layer. 

CHBr3  Layer. 

Aq.  Layer. 

CC1«  Layer. 

o-5 

36 

o-5 

33 

o-S 

15 

i 

80 

i 

66 

i 

28 

2 

I63 

2 

136 

2 

60 

3 

240 

3 

206 

3 

90 

4 

330 

4 

276 

4 

123 

5 

420 

5 

346 

5 

156 

6 

5*5 

6 

415 

6 

190 

7 

620 

8 

260 

10 

340 

12 

43° 

14 

520 

BRUCINE     C21H20(OCH3)2N2O2.4H2O. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  i8°-22°. 

(Muller  —  Apoth.  Ztg.  18,  232,  '03.) 


Solvent. 

Water 
Ether 

Acetic  Ether 
Benzene 


Gms.  Brucine 

per  100  Gms. 

Solution. 

0.0563 

0-749 
4-255 
I. II 


Solvent. 


Gms.  Brucine 

per  loo  Gms. 

Solution. 


Petroleum  Ether  0.088 

Carbon  Tetra  Chloride  0.078 
Carbon  Tetra  Chloride*  1.937 
Glycerine  2 . 2 

*  Schindelmeiser  —  Chem.  Ztg.  25,  129,  '01. 


BUTANE    C4HJ0. 

SOLUBILITY  IN  WATER  AT  t°.   AND  760  MM. 

t°.  o°  4°  10°  15°  20° 

Vols.  C4H10 
per  100  vols.  H/)  3.147        2.77        2.355        2.147        2.065 


Iso    BUTYL    ACETATE,    etc. 

SOLUBILITY  IN  WATER. 

(Traube  — Ber.  17,  2304,  '84;  at  20°,  Vaubel  — J.  pr.  Chem.  59,  30,  '99.) 


Compound. 


Grams  Com- 
pound per  100 
Grams  HzO. 


22 
22 
2O 

20 


Iso  Butyl  Acetate  0.5 

Iso  Butyl  Formate  i .  o 

Normal  Butyric  Aldehyde  3.6 

Iso  Butyric  Aldehyde  10.0 


BUTYL  ACETATE  70 

SOLUBILITY  OF  BUTYL  ACETATE  AND  OF  BUTYL  FORMATE  IN  MIXTURES 
OF  ALCOHOL  AND  WATER. 

(Bancroft  —  Calc.  from  Pfeiffer  —  Phys.  Rev.  3,  205,  'ps-'jtf.) 

cc.  H-jO  added  to  cause  separation  of  a 
AI     u  i  second  phase  in  mixtures  of  the  given 

in  Mbrture.  quantity  of  alcohol  and  3  cc.  portions  of: 


Butyl  Formate. 

Butyl  Acetate. 

3 

3-45 

2.08 

6 

8.83 

6.08 

9 

14-75 

10.46 

12 

21.45 

15-37 

11 

29.65 
39-o 

20-42 
25  .60 

21 

51.8 

3J-49 

24 

00 

37-48 

27 

43-75 

30 

50-74 

33 

59-97 

ioo  cc.  H2O  dissolve  0.7  cc.  iso  butyl  acetate  at  25°  (Bancroft). 

Iso    BUTYRIC    ACID     (CH3)2CH.COOH. 

SOLUBILITY  IN  WATER. 

(Rothmund  —  Z.  physik.  Chem.  26,  475,  '98.) 

Synthetic  Method  used,  see  Note,  p.  9. 

Gms.  Iso  Butyric  Acid  per  ioo  Gms. 


b      . 

Aq.  Layer. 

Iso  Butyric  Ac.  Layer. 

5 

16.4 

73-4 

10 

17-5 

68.5 

15 

19-4 

62.5 

20 

22.6 

53-9 

22 

25.8 

49.6 

24.7     (crit.  temp.)        36.3 

CADMIUM    BROMIDE    CdBr2. 

SOLUBILITY  IN  WATER. 

(Dietz  —  Ber.  32,  95,  '99;  Z.  anorg.  Chem.  20,  260,  '99;  Wiss.  Abh.  p.t.  Reichanstalt,  3,  433,  'oo;  see  also 
Eder  —  Dingier  polyt.  J.22I,  189,  '76;  Etard  —  Ann.  chim.  phys.  [7]  2,  536,  '94.) 

Gms.CdBr2   Mols.  CdBr2  Gms.  CdBr2   Mols.  CdBr2 

t   .  per  ioo  Gms.      per  ioo  Solid  Phase.  t°.  per  ioo  Gms.       per  ioo      Solid  Phase. 

Solution.      Mols.  H2O.  Solution.      Mols.  H2O. 

o  37.92  4.04  CdBr2.4H2O       40  60.65  10.20  CdBr2.H3O 

18  48.90  6.21  45  60.75  10.24 

30  56.90  8.73  "                60  61.10  10.39          " 

38  61.84  10.73  80  62.29  Jo-48 

35  60.29  10.05  CdBr2.H2O       ioo  61.63  IO-63          " 

Density  of  saturated  solution  at  18°=  1.683. 


7i 


CADMIUM    BROMIDE 


SOLUBILITY  OF  CADMIUM  BROMIDE  IN  ALCOHOL,  ETHER,  AND 
IN  ACETONE. 

100  gms.  sat.  solution  of  CdBr2.4H2O  in  abs.  alcohol  contain  20.93 
gms.  CdBr2  at  15°  (Eder). 

100  gms.  sat.  solution  of  CdBr2.4H2O  in  abs.  ether  contain  0.4  gm. 
CdBr2at  15°  (Eder). 

100  gms.  absolute  acetone  dissolve  1.559  gms-  CdBr2  at  18°. 

(Naumann  —  Ber.37,  4332,  '04.) 


CADMIUM    (Mono)    AMMONIUM    BROMIDE     CdBr2.NH4Br. 
SOLUBILITY  IN  WATER. 

(Rimbach  —  Ber.  38,  1553,  '05;  Eder.) 


AO                  ioo  Grams  Solution  contain  Gms. 

Atomic  Relation  .       G  .  CdBrs.NH^r 

'Cd. 

Br. 

NH4. 

Cd 

:     Br     : 

;     NH4. 

|^tl      l\J\J    VJlllD. 

Solution. 

I  -O 

16.33 

34-87 

2.63 

I 

3 

I 

53-82 

14-8 

17.40 

37-15 

2.80 

I 

3 

I 

58.01 

52.2 

19-79 

42.38 

3.21 

I 

3 

I 

65-31 

IIO.I 

22.99 

49.17 

3-72 

I 

3 

I 

75-98 

ioo  gms.  sat.  solution  of  CdBr2.NH4Br  in  abs.  alcohol  contain  15.8 
gms.  double  salt  at  15°  (Eder). 

ioo  gms.  sat.  solution  of  CdBr2.NH4Br  in  abs.  ether  contain  0.36 
gm.  double  salt  at  15°  (Eder). 


CADMIUM    (Tetra)    AMMONIUM    BROMIDE    CdBr2.4NH4Br. 

SOLUBILITY  IN  WATER. 

(Rimbach.) 

The  double  salt  is  decomposed  by  water  at  temperatures  below  160* 

ioo  Gms.  Solution  contain  Gms.      Atomic  Relation  in  Sol.       Atomic  Relation  in  Solid. 


I    . 

'    Cd. 

Br. 

NH4. 

Cd 

:     Br      : 

NH4. 

Cd 

:     Br       : 

NH4. 

0.8 

14.72 

50 

.46 

6.67 

I 

4.82 

2.82 

I 

10 

.02 

8.02 

13.0 

*4-95 

51 

.48 

6.85 

I 

4-85 

2.85 

I 

II 

•57 

9-57 

44-o 

15  .01 

53 

•85 

7-35 

I 

5-04 

3-04 

I 

6 

.84 

4.84 

76.4 

14.6 

54 

.28 

7.80 

I 

5-32 

3-32 

I 

6 

•63 

4-63 

I23-5 

J5-5 

59 

•5o 

8-45 

I 

5-38 

3-38 

I 

7 

.40 

5-4o 

160.0 

14.7 

62 

.67 

9-43 

I 

5-99 

3-99 

I 

6 

•03 

4-03 

CADMIUM  (Mono)  POTASSIUM  BROMIDE     CdBr2.KBr.H2O. 
SOLUBILITY  IN  WATER. 

(Rimbach;  see  also  Eder.) 


t°. 
0-4 

50.0 
112. 5 


ioo  Gms.  Solution  contain  Gms. 


Cd. 


Br. 


K. 


*5-4i  33-o  5-42 

16.85  35-96  5-86 

19.58  41.86  6.85 

22.24  48.28  8.14 


Atomic  Relation  in  Sol. 

Gms.CdBr2.KBr 

'Cd      : 

Br 

:      K. 

Solution. 

I 

3 

I 

53  -63 

I 

3 

I 

58.61 

I 

3 

I 

67.87 

0.98 

3 

1.03 

78.11 

CADMIUM    BROMIDE  72 

CADMIUM  Tetra  POTASSIUM  BROMIDE  is  decomposed  by  water  at 
ordinary  temperatures. 

CADMIUM    (Mono)    RHUBIDIUM    BROMIDE    CdBr2.RbBr. 
SOLUBILITY  IN  WATER. 

(Rimbach.) 


too  Gms. 

Solution  contain  Gms. 

Atomic  Relation  in  Sol  .      Gms.  CdBr2.RbBr 

t°. 

per  100  Gms. 

Cd. 

Br. 

Rb. 

Cd     : 

Br 

Rb.' 

Solution. 

0.4 

8.37 

!7-93 

6-43 

I 

3 

I  .01 

32.65 

14-5 

10.72 

23.02 

8.30 

o-99 

3 

1.  01 

41-87 

49.2 

15.01 

32.I3 

11.51 

i 

3 

I 

58-54 

107-5 

19.65 

41.12 

14.06 

1.02 

3 

0.96 

75-77 

CADMIUM    (Tetra)    RHUBIDIUM    BROMIDE    CdBr2.4RbBr. 
SOLUBILITY  IN  WATER. 

(Rimbach.) 
too  Gms.  Solution  contain  Gms.  Atomic  Relation  in  Sol.    Gms.CdBr2.4RbBr 


13-5 
114-5 


CADMIUM    (Mono)    SODIUM    BROMIDE    CdBr2.NaBr2iH3O. 
SOLUBILITY  IN  WATER,  ETC.,  AT  15°. 

(Eder  — Ding,  polyt.  J.  221,  189,  '76.) 

Gms.  CdBr2.NaBr  per  100  Gms.  Solid 

° VCn  '  'Solution.  Solvent.'  Phase. 


Cd 

Br 

Rb. 

Cd     : 

Br 

:      Rb.' 

per  100  «jm 
Solution. 

5-70 

24.94 

17.97 

0.98 

6 

4-05 

47-95 

6-55 

28.74 

20-74 

o-97 

6 

4-05 

55-J7 

8.25 

35  -51 

25-39 

0.99 

6 

4-02 

68.82 

9-5° 

40.67 

29.00 

1.  00 

6 

4.0 

79-04 

Water  49.0  96.1  CdBr2.NaBr.2^H2O 

Absolute  Alcohol          21.2  27.0 

Absolute  Ether  0.52  0.53 


CADMIUM    CHLORATE    Cd(ClO3)2.2H2O. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  35,  1422,  '02.) 

Gms.  Mols.  Gms.  Mols. 

t«       Cd(C103)2      Cd(C103)2          Solid  Phase  f    Cd<a<£>»     Cd(ClO3)2         Solid  Phase. 

per  100  Gms.  per  100  Mols.         °        ruasc.  *  'periooGms.     per  100 

Solution.  H2O.  Solution.      Mols.H2O. 

-20    72.18        22.47    Cd(ClO3)2.2H2O   18    76.36        27.98Cd(ClO3)2.2H2O 
-15     72.53        22.87  49    80-08        34-82 

o    74-95        25.92  65    82.95        42-14 

Density  of  the  saturated  solution  at  18°  =  2.284. 


73 


CADMIUM    CHLORIDE 


SOLUBILITY  IN  WATER. 

(Dietz  —  W.  Abh.  p.  t.  Reichanstalt  3,  433,  'oo;  above  100°,  Etard  —  Ann.  chim.phys.t?]  2,  536,  '94.) 


t  °. 

G.  CdCl2  perMols.CdC!2         Soiid 
100  Gms.        per  100            p,                           t  °. 
Solution.    Mols.H2O. 

G.CdCl,per 
100  Gms. 
Solution. 

Mols.CdCl,          s^ 

iffi/Sb.     *5. 

-  9 

43-58 

7-5] 

+  10 

57-47 

*3-3 

0 

49-39 

9.6 

PHri     TT  O        2O 

57-35 

13.2 

+  10 

55-58 

12.3 

40 

57-51 

13-3 

I5 

59.12 

14-  2J 

60 

57-7i 

13-4 

—  10 

44-35 

7-8^ 

80 

58.41 

13.8 

o 

47-37 

9.0 

100 

59-52 

14-4. 

+  18 

52-53 

10.9 

^CdCl2.2iH20    150 

64.8 

3° 

56.91 

12.8 

(monoclinic)            2OO 

72.0 

36 

57-91 

13-5. 

270 

77-7 

Density  of  saturated  solution  at  18°  =  1.741. 

100  gms.  abs.  ethyl  alcohol  dissolve  1.52  gms.  CdCl2  at  15°.  5. 
100  gms.  abs.  methyl  alcohol  dissolve  1.71  gms.  CdCl2  at  15°.  5. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  783,  '92.) 

CADMIUM    AMMONIUM    CHLORIDE    CdCl2.NH4Cl. 

SOLUBILITY  IN  WATER. 

(Rimbach  —  Ber.  30,  3075,  1897.) 
100  Gms.  Solution  contain  Gms.  Gms.  CdC^.NHiCl  per  100  Gms. 


i>  . 

Cd. 

Cl. 

NH  . 

Solution. 

Water.  ' 

2.4 

14.26 

13-44 

2  .24 

29-94 

42.74 

16.0 

15.82 

15-07 

2.56 

33-45 

50.26 

41.2 

18.61 

17.46 

2.89 

38.96 

63  -83 

63.8 

20.92 

19-73 

3-34 

43-99 

78.54 

105.9 

24.70 

23-52 

4.01 

52-23 

109.33 

CADMIUM    (Tetra)    AMMONIUM    CHLORIDE    CdCl2.4NH4Cl. 

IN  CONTACT  WITH  WATER. 
The  salt  is  decomposed  in  aqueous  solution. 

(Rimbach.) 
.  o  100  Gms.  Solution  contain  Gms.  Atomic  Relation  in  Solution. 


* 

'    Cd. 

Cl. 

NH4.                 C 

d      :      Cl      : 

NIL; 

3-9 

5-75 

18.17 

7-37 

9-96 

7.96 

16.1 

6.96 

20.26 

7-97 

9-2O 

7-13 

40.2 

9.91 

23.84 

8.92 

7.6i 

5.61 

58-5 

12.50 

26.53 

9-35 

6.7i 

4.66 

112  .9 

16.66 

3J-79 

10.78 

6.  02 

4.02 

iJ3-9 

16.51 

32.71 

11.30 

6.26 

4.26 

SOLUBILITY  OF  MIXTURES  OF  CADMIUM  TETRA  AMMONIUM  CHLORIDE 
AND  CADMIUM  AMMONIUM  CHLORIDE  IN  WATER. 

(Rimbach  —  Ber.  35t  1300,  '02.) 


100  Gms.  Solution  contain  Gms. 

Atomic  Relation. 

Solid  Phase, 
Mol.  per  cent  of: 

Cd. 

Cl. 

NH4. 

Cd 

:    Cl       : 

NH*. 

CdCli. 
NH«CL 

CdClj. 
4NH4C1. 

I  .1 

5-34 

17.62 

7.27 

i 

10-47 

8.50 

49.6 

50-4 

14.0 

7.12 

19.86 

7.84 

i 

8.84 

6.87 

47-0 

53-o 

40-7 

10.24 

23  .82 

8.85 

i 

7-37 

5-37 

77.0 

23  o 

58.5 

12.50 

26-53 

9-35 

i 

6.7I 

4.66 

CADMIUM    CHLORIDE 


74 


SOLUBILITY  OP  MIXTURES  OF  CADMIUM  TETRA  AMMONIUM  CHLORIDE 
AND  AMMONIUM  CHLORIDE  IN  WATER. 

(Rimbach.) 


ioo  Gms.  Solution 
40                        contain  Gms. 

Atomic 
Relation  . 

Solid  Phase, 
Mol.  per  cent  of: 

Cd. 

Cl. 

NH. 

Cd 

:     Cl       : 

NH4. 

NH4C1.    CdCl2.4NH4Ci. 

I  -0 

2.82 

17.11 

7 

.82 

I 

19 

.21 

17.28 

59-o 

41 

.0 

I3.2 

2.76 

18.84 

8 

.71 

I 

21 

.62 

19.62 

74-0 

26 

.0 

4O.I 

3.16 

22  .56 

10 

•49 

I 

22 

•65 

20-74 

71.0 

29 

.0 

58-2 

3-51 

25.21 

II 

.72 

I 

22 

•79 

20.89 

69.0 

31 

.0 

CADMIUM    BARIUM    CHLORIDE    2(CdCl2).BaCl2.sH2O. 
SOLUBILITY  IN  WATER. 

(Rimbach  —  Ber.  30,  3083,  '97.) 


ioo  Gms.  Solution 

Gms.  2(CdCl2).BaCl2 

t°. 

contain  Gms. 

per  ioo  Gms. 

Cd. 

Cl. 

Ba. 

Solution. 

Water. 

22  .6 

17.71 

16.89 

II  .0 

45-60 

83.82 

41-3 

19.22 

18.15 

11-77 

49.14 

96.62 

53-9 

19.85 

18-75 

12.41 

51.04 

104.25 

62.2 

20-59 

19.66 

12.83 

53-08 

"3-13 

69  5 

21  .20 

20.  18 

13.09 

54-47 

119.64 

107.2 

24.25 

23-23 

14.90 

62.38 

165-85 

CADMIUM    BARIUM    CHLORIDE    CdCl2.BaCl2.4H2O. 
SOLUBILITY  IN  WATER. 

(Rimbach.) 


ioo  Gms.  Solution 

Gms.  CdCl2.BaCl2 

t°. 

contain  Gms. 

per  ioo  Gms. 

Cd. 

Cl. 

Ba. 

Solution.             Water. 

22.5 

11.98 

15.19 

14.71 

41.88              72.06 

32-9 

12  .40 

16.18 

16.09 

44.67              80.73 

41.4 

I3-05 

16.95 

16.81 

46.81          88.01 

S3  -4 

13.96 

18.21 

18.13 

50.30         101.21 

62  .0 

J4-73 

18.81 

18.74 

52.28         109.56 

97-8 

17-57 

22.48 

22.00 

62.05         l63-^o 

108.3 

18-53 

23-51 

22.79 

64.83         184.33 

109.2 

18.67 

23.69 

29-95 

65.31         188.27 

CADMIUM   MAGNESIUM  CHLORIDE    2(CdCl2)MgCl2.i2H2O. 
SOLUBILITY  IN  WATER. 

(Rimbach.) 


ioo  Gms. 

Solution 

Gms.  2(CdC 

l2).MgCl2 

1;*.                                    contain  Gms. 

per  ioo  l 

jms. 

Cd. 

Cl. 

Mg. 

Solution. 

Water. 

2 

•4 

22 

,14 

21  . 

06 

2 

.41 

45 

,6l 

83.86 

2O 

.8 

24 

30 

22  . 

80 

2 

•55 

49 

,69 

98.77 

45 

•5 

26 

.24 

24- 

55 

2 

.72 

53 

51 

115.10 

67 

.2 

28 

45 

26. 

7i 

2 

.98 

58 

,14 

138.90 

121 

.8 

31 

.84 

30 

20 

3 

•44 

65 

,48 

189    69 

75  CADMIUM    CHLORIDE 

CADMIUM  (Mono)  RHUBIDIUM  CHLORIDE  CdCl2.RbCl. 
SOLUBILITY  OF  CADMIUM  MONO  RHUBIDIUM  CHLORIDE  IN  WATER. 

(Rimbach  —  Ber.  35,  1303,  '02.) 
100  Gms.  Solution    ontain  Gms.  Gms.  CdCl2.RbCl  per  100  Cms. 


I/     . 

Cd. 

Cl. 

Rb. 

Solution. 

Water. 

I  .2 

4.80 

4-53 

3-63 

12-97 

14.90 

14-5 

6.20 

5.88 

4-75 

16.80 

2O.I9 

41.4 

9-34 

8.86 

7.14 

25-31 

33  89 

57-6 

ii  .40 

10.78 

8.63 

30-83 

44  -58 

103.9 

17.14 

16.37 

13-39 

46.62 

87.36 

CADMIUM    (Tetra)    RHUBIDIUM    CHLORIDE    CdCl2.4RbCl. 
IN  CONTACT  WITH  WATER. 

(Rimbach.) 

The  double  salt  decomposes  to  CdCl2.RbCl  and  RbCl. 


t  ° 

100  Gms. 

Solution  contain  Gms. 

Atomic  Relation. 

Solid  Phase, 
Mol.  per  cent  of: 

Cd. 

Cl. 

Rb. 

Cd     :      Cl 

:      Rb. 

CdCl2. 
RbCl. 

Cdc;i2. 

4RbCl. 

o-7 

0.65 

6.52 

J4-73 

I       31.88 

29.88 

30 

70 

8.8 

1.07 

7-37 

16.13 

I       21.89 

19.89 

24 

76 

13.8 

1.32 

7.86 

16.93 

I       18.88 

16.83 

16 

84 

42.4 

3-21 

n-35 

22.45 

I       II  .21 

9.21 

14 

86 

59-o 

4.61 

13  .41 

25-31 

I          9.23 

7-23 

33 

67 

108.4 

8.94 

18-57 

3I-I5 

I          6.57 

4-59 

SOLUBILITY  OF  MIXTURES  OF  CdCl2.4RbCl  AND  RbCl  IN  WATER. 

(Rimbach.) 

100  Gms.  Solution  contain  Gms.  Atomic  Relation.          Mo?°per  cent'of : 

Cd!  CL~  Rb!"  Cd     !~C1  :     Rb.      CdCl2.4Rbcl RbCl. 

0.4  12.86        30.97         ..ii  55          45 

14.8  13.62        32.81         ..       i       i  67          33 

17.9  14.0          33.71         ..       i       i  80          20 

THE  EFFECT   OF   THE   PRESENCE  OF  HC1,  CaCl2  AND   OF   LiCl  UPON 

THE  DECOMPOSITION  OF  CADMIUM  TETRA  RHUBIDIUM 

CHLORIDE  BY  WATER  AT  16°. 

(Rimbach  —  Ber.  38,  1570,  '05.) 
100  Gms.  Solution  contain  Gms.  Mols          IQQ  Mds  HZQ        MoieCular  Ratio. 


Total  Cl. 

Cl. 

HCl. 

Cd. 

Rb. 

CdCl2. 

RbCl. 

HCl.      CdCla 

:     RbCl. 

36-44 

0-84 

36.61 

0.41 

I 

•39 

O 

109 

0-483 

29.76 

I 

4-43 

28.45 

0.8o 

28.44 

o-35 

I 

•38 

o 

.082 

0.422 

20-35 

I 

5^5 

12  .09 

3-24 

9.11 

0.69 

6 

•74 

0 

•I39 

1.772 

5.60 

I 

12-75 

Ca. 

CaCl2. 

CaCl2. 

14.98 

7-56 

20.91 

o-73 

2 

.80 

o 

•159 

0-799 

4-59 

I 

5-04 

12.70 

5-77 

15.96 

0.77 

4 

.87 

o 

.163 

i-353 

3-4i 

I 

8.31 

10.85 

3-78 

14.47 

i  .00 

8 

•51 

0 

.211 

2-365 

2.24 

I 

II  .22 

9-o8 

1.84 

5.10 

1.24 

12 

.14 

o 

.262 

3-385 

1.09 

I 

12.92 

Li. 

LiCl. 

LiCl. 

26.49 

4-87 

29.40 

0.56 

3- 

871 

o 

•139 

i  .271 

19.40 

I 

9-J3 

20-37 

3-33 

2O    II 

0-52 

7- 

84 

0 

.122 

2-433 

12.54 

I 

19.88 

See  Note  on  next  page. 


CADMIUM    CHLORIDE  76 

CADMIUM    (Mono)    POTASSIUM    CHLORIDE    CdCl2.KCl.H2O. 
SOLUBILITY  IN  WATER. 

(Rimbach —  Ber.  30,  3079,  '97;  see  also  Croft  —  Phil.  Mag.  [3]  21,  356,  '42.) 

100  Cms.  Solution  Cms.  CdCl2.KCl 

^o_  contain  Gms.  per  100  Gms. 

Cd.  Cl £.  Solution.  Water. 

•       2.6          9.53          9.03        3.31  21.87          27.99 

15.9  11-63  10-98  3.99  26.60  36-24 

41.5  15.47        14-73        5-45  35 -66          55-34 

60.6  17.68         16.80        6.20  40.67          68.55 
105.1         22.46        21.34        7.87  5J-67         106.91 


CADMIUM    (Tetra)    POTASSIUM    CHLORIDE    CdCl2.4KCl. 
IN  CONTACT  WITH  WATER. 

(Rimbach.) 

The  double  salt  is  decomposed  when  dissolved  in  water  at  ordinary 
temperature. 

TOO  Grams  Solution  contain  Gms. 


l<    . 

Cd. 

Cl. 

K. 

4 

3-64 

9.84 

8.3I 

23.6 

5.66 

14.02 

11.52 

50.2 

9.10 

18.09 

13.60 

108.9 

11.94 

23.11 

17  .16 

NOTE.  —  The  effect  of  the  presence  of  certain  chlorides  upon  the 
decomposition  of  cadmium  tetra  potassium  chloride  by  water  at  16° 
was  investigated  by  Rimbach  in  a  manner  similar  to  that  used  in  the 
case  of  cadmium  tetra  rhubidium  chloride  (see  preceding  page).  The 
results,  which  show  the  extent  to  which  increasing  amounts  of  the 
several  chlorides  force  back  the  decomposition  of  the  double  salt,  were 
plotted  on  cross-section  paper,  and  the  points  at  which  the  decom- 
position was  prevented,  were  determined  by  interpolation.  These 
values  which  show  the  minimum  amount  of  the  added  chlorides  which 
must  be  present  to  insure  the  crystallization  of  the  pure  double  salt  are 
shown  in  the  following  table. 


Added 

Mols. 

per 

ioo  Mols 

.  H20. 

Density  of 

Mols. 

per 

Liter  of 

Solution. 

Chloride. 

CdCl2. 

KC1. 

Added 
Chloride. 

Solutions. 

CdCl2. 

KC1. 

Added* 
Chloride. 

HC1 

0.074 

0 

.296 

19 

.80 

I 

.1403 

0-033 

0 

.132 

8.828 

LiCl 

0-344 

I 

•376 

9 

•30 

I 

.1380 

0.166 

0 

.663 

4.483 

CaCIg 

0-544 

2 

.I76 

3 

.80 

I 

•2333 

0.270 

I 

.808 

1.887 

KC1 

1.034 

6 

.514* 

2 

•378 

I 

.214 

0.507 

3 

.195* 

I  .167 

*  Total. 

CADMIUM    CYANIDE    Cd(CN)2. 

ioo  gms.  H2O  dissolve  1.7  gms.  Cd(CN)2  at  15°. 


(Joannis  —  Ann.  chim.  phys.  [5]  26,  489,  '82.) 


77 


CADMIUM    FLUORIDE 


CADMIUM    FLUORIDE    CdF2. 

SOLUBILITY  IN  WATER. 
100  cc.  saturated  aqueous  solution  contain  4.36  gms.  CdF2  at  25°. 

(Jager  —  Z.  anorg.  Chem.  27,  34,  'ox.) 

CADMIUM    HYDROXIDE    Cd(OH)2. 

SOLUBILITY  IN  WATER. 
i  liter  of  aqueous  solution  contains  0.0026  gm.  Cd(OH)2  at  25°. 

(Bodlander  — Z.  physik.  Chem.  27,  66,  '98.) 

CADMIUM    IODIDE    CdI2. 

SOLUBILITY  IN  WATER. 

(Dietz  —  W.  Abh.  p.  t.  Reichanstalt  3,  433,  'oo;    see  also  Kremers  —  Pogg.  Ann.  103,  57,  '58;  Eder 
—  Dingl.  polyt.'  J.  221,  189,  '76;  Etard —  Ann.  chim.  phys.  [7]  2,  536,  '94.) 


A0      Gms.  CdI2  per  100  Gms. 

Mols.  CdI2 

Gms.  CdI2  per  100  Gms. 

Mols.  CdI2 

Solution. 

Water. 

MoTs!H°2O. 

Solution. 

Water. 

per  100 
Mols.  H2O. 

0 

44.4 

79-8 

3-9 

30 

47-3 

89.7 

4-43 

10 

45-4 

83.2 

4.1 

40 

48.4 

93-8 

4.6 

15 

45-8 

84-5 

4.17 

50 

49-35 

97-4 

4.8 

18 

46.02 

85.2 

4.2 

75 

52-65 

III  .2 

5-4 

20 

46-3 

86.2 

4.26 

100 

56.08 

127.6 

6-3 

25 

46.8 

87.9 

4-34 

Density  of  saturated  solution  at  18°  =  1.590. 


SOLUBILITY  OF  CADMIUM  IODIDE  IN  ORGANIC  SOLVENTS. 


Observer. 

(Eder.) 

(Timofeiew  —  Compt.  rend.  112,  1224,  '91.) 
(Timofeiew  —  Compt.  rend.  112,  1224,  '91.) 
(Timofeiew  —  Compt.  rend.  112,  1224,  '91.) 

(Eder.) 
(Naumann  —  Ber.  37,  4332,  '04.) 


Gms.  CdI2  per 

Solvent. 

t°. 

TOO 

Gms. 

Solution. 

Solvent. 

Absolute  Alcohol 

15 

50-5 

102.0 

Ethyl  Alcohol 

20 

42  .6 

74.27 

Methyl  Alcohol 

20 

59-o 

*43-7 

Propyl  Alcohol 

2O 

28.9 

40.67 

Absolute  Ether 

15 

21.7 

27.7 

Absolute  Acetone 

18 

20-0 

25.0 

CADMIUM  AMMONIUM    IODIDES    (Mono  and  Di) . 
SOLUBILITY  IN  WATER,  ETC. 

(Rimbach  —  Ber.  38,  1557.  '05;  at  15°  Eder  —  Dingl.  polyt.  J.  221,  189,  '76.) 


Solvent. 

Water 

Abs.  Alcohol 

Abs.  Ether 


Cd.  Mono 
Ammonium  Iodide. 

Gms.  CdI2.NH4I  per 
t°  100  Gms. 


15 


Solution.  Solvent. 

52.6  ni.o 

53  JI3 
29.4          41-7 


Cd.  Di 
Ammonium  Iodide. 


Gms.  CdI2.2NHJ  per 
t°.                        100  Gms. 

Solution. 

Solvent. 

14-5 

85-97 

6II.6 

15 

59 

143 

IS 

10 

II 

CADMIUM    IODIDES  78 

CADMIUM    POTASSIUM   IODIDES,  Mono  =  CdI2.KI.H2O, 
Di=  CdI2.2KI.2H2O. 

CADMIUM    Di    SODIUM    IODIDE    CdI2.2NaI.6H2O. 

SOLUBILITY  IN  WATER,  ETC.,  AT  15°. 

(Eder.) 


Gms.  CdI2.KI 
Solvent.                      ***  I0?  Gms" 

Gms.  CdI2.2KI 
per  100  Gms. 

Gms.  CdI2.2NaI 
per  100  Gms. 

Solution. 

Solvent. 

Solution. 

Solvent. 

Solution. 

Solvent. 

Water               51.5 
Abs.  Alcohol 
Abs.  Ether 

1  06 

57-8 
41.7 

3-9 

137 
71 
4.1 

6l.3 

53-7 
9.0 

158.8 

116.2 
9-9 

CADMIUM    NITRATE    Cd(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3   440,  'oo.) 


Gms.  Cd(N03)2 
t  o_                     per  100  Gms. 

Solution. 

Water. 

-13 

37-37 

59-67 

—     I 

47-33 

89.86 

+     I 

52-73 

III-5 

0 

52-37 

109.7 

+  18 

55-9 

126.8 

30 

58-4 

140.4 

40 

61  .42 

159.2 

59-5 

76-54 

326-3 

25.0 

Density  of  saturated  solution  at  18°  =  1.776. 


Mols.  Cd(NO3)2 

Solid 

per  100  Mols.  H2O. 

Phase. 

4-55 

Cd(N03)2.9H20 

6.85 

" 

8.50 

" 

8-37 

Cd(NOs)2.4H20 

9.61 

" 

10-7 

" 

12  .1 

tt 

K 

CADMIUM    OXALATE    CdC2O4.3H2O. 

i  liter  of  sat.  aqueous  solution  contains  0.033  gm-  CdC2O4  at  18°. 

(Kohlrausch  —  Z.  physik.  Chem.  44,  197,  '03.) 

CADMIUM    SULPHATE    CdSO4. 

SOLUBILITY  IN  WATER. 

(Mylius  and  Funk  —  W.  Abh.  p.  t.  Reichanstalt  3,  444,  'oo;  see  also  Kohnstamm  and  Cohn  —  Wied 
Ann.  65,  344,  '98;  Steinwehr  —  Ann.  der  Phys.  (Drude)  [4]  Q,  1050,  '02;  Etard  • — Ann.  chim.  phys 
[7]  2  536,  '94.) 


Solid 


Gms.  CdSO4 
t  °.             per  TOO  Gms. 

Solution. 

Water. 

-17 

44-5 

80.2 

—  10 

46.  i 

85.5 

-  5 

48.5 

94-2 

-18 

43-35 

76.52 

—  10 

43-27 

76.28 

0 

43.01 

76.48 

+  10 

43.18 

76.00 

20 

43-37 

76.60 

CdS04.7H20 


CdSO4.|H2O 


40 
60 
73-5 
74-5 
77 
85 
90 

100 

Gms.  CdSO4 
per  100  Gms. 

Solid 

CdSO4.fH2O. 
tt 

CdS04.H2O 
it 

it 
it 
tt 

Solution.  Water. 

43-99  78.54 

44.99  83.68 
46.6  87.28 

46.7  87.62 

42.2  73.02 

39-6  65.57 
38.7  63.13 
37.8  60.77 

79 


CADMIUM    SULPHATE 


SOLUBILITY  OF  CADMIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  SUL- 
PHURIC ACID  AT  o°. 

(Engel  — Compt.  rend.  104,  507,  '87.) 


Equivalents  per  10  Gms.  H2O. 


H2S04. 

CdSO4. 

o. 

71.6 

3-87 

70.9 

12.6 

62  .4 

28.1 

50.6 

43-3 

40.8 

47.6 

37-o 

53-8 

32-7 

7i-5 

23.0 

Density 
of  Solutions. 

I  .609 


Grams  per  100  Grams  H2O. 


545 

476 

435 
421 
407 
379 


H2S04. 

CdSO4. 

O-OO 

74.6l 

I  .90 

73-87 

6.18 

65-°3 

I3-78 

52-73 

21.23 

42.52 

23-34 

38-56 

26.38 

34-07 

35-06 

23.96 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  CADMIUM  SULPHATE  AND  FERROUS 
SULPHATE  IN  WATER  AT  25°. 

(Stortenbecker  —  Z.  physik.  Chem.  34,  109,  'oo.) 


Composition  of  Solution. 


Gms.  per 

100  Gms.  H2O. 

Mols.  per  : 

too  Mols.  H2O. 

Mol.  %  Cd. 

CdSO4. 

FeSO4. 

Cd. 

Fe.       ' 

in  Sol. 

Crystals  with  2§  Mols.  H2O. 

76.02 

o.o 

6-57 

o.o 

100 

57-6i 

10.63 

4-98 

1.26 

79-8 

Crystals  with  7 

Mols.  H20. 

57-6i 

10.63 

4.98 

1.26 

79-8 

78.5 

44-6 

24.4 

0-0 

26.60 

o.o 

3-I65 

o.o 

Mol.  per  cent  Cd  in 
Crystals  of 
Solid  Phase. 


100 

99-o 

36.6 
34-6 
ii  .1 

4-8 
o.o 


CADMIUM    POTASSIUM    SULPHATE     CdK2(SO4)2. 
SOLUBILITY     IN     WATER. 

(Wyrouboff  —  Bull.  soc.  chim.  [3]  25,  121,  '01.) 


to 

G.  CdK2(S04): 

i  per 

Solid 

to 

G.  CdK2(SO4)2 

, 

100  Gms.  H2( 

) 

Phase. 

. 

per  100  Gms.  H2O. 

16 

42.89 

CdK2 

(S04)2.2H20 

26 

42.50      C 

31 

46.82 

" 

31 

42.80 

40 

47-40 

a 

40 

43-45 

64 

44.90 

Solid 
Phase. 


CdK2(S04)2.iiH20 


CADMIUM  SODIUM 
SULPHATE 


80 


CADMIUM    SODIUM    SULPHATE    CdNa2(SO4)2.2H2O. 

SOLUBILITY  IN  WATER,  ALSO  WITH  THE  ADDITION  OF  CADMIUM  SUL- 
PHATE  AND  OF  SODIUM  SULPHATE. 

(Koppel,  Gumpery  —  Z.  physik.  Chem.  52,  413,  '05.) 


Solid  Phase. 


CdNa2(S04)2.2H20 


CdNa2(SO4)2.2H2O 
+  CdSO|.|H20 


CdNa2(SO4)2.2H2O 
+  Na2S04.ioH20 


CdNa2(SO4)2.2H2O 
+Na2SO4 


Gms.  per  100  Gms. 
40.               Solution. 

Gms.  per  100  Gms. 
H20. 

Mols.  per  100  Mols. 
H20. 

24 
30 

CdS04. 
22.25 

22-55 

Na2SO4. 

I5-07 
15.29 

CdSO4. 

35-49 
36.28 

Na2S04. 
24.04 
24.60 

CdS04.     Na2S04. 
3-07      3-05) 

3-J4    3-12  Y 

40 

22.89 

15  .65 

37-24 

25-45 

3.22     3-28; 

O 

40.32 

4-85 

73-54 

8.85 

6.36 

1 

10 

39  -91 

5-24 

72.77 

9-55 

6.30 

.21    1 

20 

40.26 

5-16 

73  -81 

9-45 

6-39 

.20 

40 

39  -89 

7.l8 

75-38 

I3-56 

6.52 

72 

•14.8  40.18 

4.60 

72.68 

8-32 

6.29 

/ 

0 

37-30 

6-53 

66.32 

ii  .62 

5-74 

•47] 

10 

32-53 

8.69 

55-34 

14-78 

4-79 

.84  I 

20 

22  .69 

14.71 

36-25 

23-52 

3.14     2.98  1 

25 

16-33 

19.82 

25.60 

31.06 

2.21     3.94' 

30 

9-21 

27.80 

14.62 

44.14 

1.26     4.59] 

35 

8.26 

29-35 

13.26 

47-06 

i  .15     5.96  [- 

40 

9.98 

28.27 

16.24 

46.27 

1.41     5.86j 

CAESIUM    ALUMS 

SOLUBILITY  OF  CAESIUM  CHROMIUM  ALUM,  CAESIUM  IRON  ALUM, 
CAESIUM  INDIUM  ALUM,  AND  OF  CAESIUM  VANADIUM  ALUM  IN 
WATER. 

(Locke  —  Am.  Ch.  J.  27,  174,  '01.) 


Formula  of  Alum. 

Cs2Cr2(S04)4.24H20 
« 

a. 
a 

Cs-Fe2(SO4)4.24H2O 


Cs2V2(S04)2.24H20 


25 
30 

35 
40 

25 
30 
35 
40 

25 
25 


Gms.  per  100  cc.  H2O. 

Anhydrous 
Salt. 

Hydrated 
Salt. 

0-57 
0.96 
I.  206 

o-94 
1.52 

x-53 

2-43 

1.71 

2.72 

2  -52 

3-75 
6.04 

4.01 
6.01 
9.80 

7-57 

n-73 

0.771 

I-31 

Gram  Mols.  Salt  per 
100  cc.  H2O. 

O.OOI5I 

O.OO25 

0.0032 

o . 00405 

O.OO45 
O.OO66 
O.OO99 
0.0156 
0.0172 
O-OO2O4 


8i         CAESIUM    CHLORAURATE 

CAESIUM    OHLORAURATE    CsAuCl4. 

SOLUBILITY  IN  WATER. 

(Rosenbladt  — Ber.  19,  2537,  '86.) 


t». 

Gms.  CsAuCl4 
per  ioo  Gms. 
Solution. 

to. 

Gms.  CsAuCU 
per  ioo  Gms.     t  °. 
Solution. 

Gms.  CsAuCU 
per  ioo  Gms. 
Solution. 

10 

o-5 

40 

3-2               80 

I6.3 

20 

0.8 

50 

5-4          90 

21.7 

30 

I-7 

60 

8.2             IOO 

27-5 

70 

12  -O 

CAESIUM    FLUOBORIDE    CsBFl4. 

100  grams  water  dissolve  0.92  gram  CsBFl4  at  20°,  and  0.04  gram 

at  100°.  (Godeffroy  —  Ber.  9,  1367,  '76.) 

CAESIUM    MERCURIC    BROMIDE    CsBr.2HgBr2. 

100  grams   saturated   aqueous    solution  contain   0.807  gram  CsBr. 

2HgBr2   at    l6°.  (Wells  -  Am.  J.  Sci.  [3}  44,  221,  '92.) 

CAESIUM    CARBONATE    Cs2CO3. 

100  grams  absolute  alcohol  dissolve  n.i  grams  Cs2CO    at  19°,  and 

20.1  grams  at  b.  pt.  (Bunsen.) 

CAESIUM    CHLORIDE    CsCl. 

SOLUBILITY  IN  WATER. 

(Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203  A,  208,  '04;  see  also  Hinrichsen  and  Sachsel  —  Z.  physik. 
Chem.  50,  99,  '04- '05;  at  25°,  Foote.) 


to 

G.  CsCl  per  IPO  Gms. 

G.Mol.CsCl 

G.  CsCl  per  ioo  Gms. 

G.  Mol.  CsCl 

. 

Solution. 

Water. 

per  Liter. 

' 

Solution 

.     Water. 

per 

Liter. 

O 

61-7 

161 

•4 

6 

•74 

60 

69 

•7 

229.7 

8 

.28 

10 

63.6 

174 

•7 

fj 

.11 

70 

70 

.6 

239-5 

8 

.46 

20 

65.I 

186 

•5 

>j 

•38 

80 

71 

•4 

250-0 

8 

-64 

3° 

66.4 

197 

•3 

7 

63 

90 

72 

.2 

26o.I 

8 

.80 

40 

67-5 

208 

.0 

h 

.86 

IOO 

73 

.0 

270.5 

8 

,96 

So 

68.6 

218 

•5 

8 

.07 

119.4 

74 

4 

290.0 

9 

.22 

SOLUBILITY    OF    MIXTURES    OF    CAESIUM    CHLORIDE    AND    MERCURIC 
CHLORIDE  IN  WATER  AT  25°. 

(Foote  —  Am.  Ch.  J.  30,  340,  '03.) 

Gms.  per  ioo  Gms.  Gms.  per  ioo  Gms. 

Solution.  Solid  Phase.  Solution.  Solid  Phase. 

CsClI  HgCl2.  CsCl2.         HgCl2. 

65.61  o.o  CsCl  38.63  1.32 

65.78          0.215         CsCl  +  CssHgCl5  17.03  0.51 

62.36  0.32  )     Double  Salt  I'S3  °'42 

57.01  0.64  I     CssHgClg  0.6l  2.64         CsHg       +  CsHg,Cl6 

52.35  1.23  )  -65-1%  CsCl  0.49  2>9I    )     DoubleSalt 

J 


51.08  1.44  Cs3HgClfi  +  CsjHgCl*  0.40  3-78  J     CsHg2Cl5  =  23.7%CsCl 

40.30  1.49      )     DoubleSalt  0.44  4.63         CsHgaClB  +  CsHg8Clu 

45.95  1.69      f     CsiHgCl4=5S.4%CSCl  0.41  4-68  )     Doubiesalt 

45-23  J-73  Cs,HgCU  +  CsHgCl,  0.25  5.65  )     CsHg8Cln=ii.i%C6Cl 

o.i  8  7.09         CsHg6Clu  +  HgCl, 

0.0  6.90         HgCl, 


CAESIUM    CHLORTELLURATE    82 

CAESIUM    CHLORTELLURATE    CsTeCl6. 

SOLUBILITY   IN  AQUEOUS  HYDROCHLORIC  ACID. 

(Wheeler  — Am.  J.  Sci.  [3]  45,  267,  '93.) 

ioo  parts  HC1  (Sp.  Gr.  1.2)  dissolve  0.05  part  CsTeCl6  at  22°. 
ioo  parts  HC1  (Sp.  Gr.  1.05)  dissolve  0.78  part  CsTeCl6  at  22°. 

CAESIUM    THALLIC    CHLORIDE    3CsCl.TlCl3.2H2O. 

ioo  parts  H2O  dissolve  2.76  parts  3CsCl.TlCl3.2H2O  at  17°,  and  33.3 

parts  at  I00°.  (Godeffroy  —  Z.  Osterr.  Apoth.  Ver.  No.  9,  1886). 

CAESIUM    IODATE    CsIO3. 

ioo  parts  H2O  dissolve  2.6  parts  CsIO3  at  24°,  and  2.5  parts  2CsIO3. 

I2O6  at  2  1°.  (Wheeler  —  Am.  J.  Sci.  [3]  44,  123,  '92.) 

CAESIUM    IODIDE    Csl. 
SOLUBILITY  OF  MIXTURES  OF  CAESIUM  IODIDE  AND  IODINE  IN  WATER. 

(Foote  —  Am.  Ch.  J.  29,  210,  '03.) 


t  °. 

-4 
-4 
—  4 

—  O-2 

Gms.  per  ioo  Gms. 
Solution.                               t°. 

Gms.  per  ioo  Gms. 
Solution. 

Solid  Phase  at 

Csl 
Csl  and  CsI3 
CsI3  and  CsI5 
CsI5  and  I 

Csl. 
27.68 
27.52 
3.l8 
0.85 

I. 
O-O 
0.09 
0.31 

0-34 

35-6 
35-6 
35-6 
35-6 

Csl. 
51.48 
51.66 
10.72 

3-74 

i. 
o.o 
0.71 
1.78 

1.  60 

Gms.  per  ioo  Gms. 
t  °                      Solution. 

In  Separated  Heavy  Solution 
Gms.  per  ioo  Gms.  Solution. 

Solid 
Phase 

Csl. 

i. 

Csl. 

] 

52 

.2 

16 

•75 

4-52 

CsI3 

and 

CsI6 

52 

.2 

6 

,69 

. 

. 

CsI5 

and 

I 

52 

.2 

6 

.72 

3-32 

22 

94 

73 

•72 

CsI5 

52 

.2 

6 

65 

3-45 

22 

.80 

.63 

I 

73 

26 

.98 

I5-07 

CsI3 

and 

CsI6 

73 

16 

.66 

10.50 

27.56 

68 

.40 

CsI5 

73 

6 

,27 

4.08 

*7 

.68 

80 

.02 

I 

CAESIUM    (Tri)  IODIDE    CsI3. 

ioo  cc.  saturated  aqueous  caesium  iodide  (about  17  per  cent  Csl) 
solution  contain  0.97  gram  CsI3  at  20°,  density  of  solution  =  1.154. 

(Wells  — Am.  J.  Sci.  [3]  44,  221,  '92.) 

CAESIUM    NITRATE     CsNO3. 

SOLUBILITY  IN  WATER. 

(Berkeley  —  Trans.  Roy.  Soc.  (Lond  )  203    A,  213,  '04.) 


Gms.  CsNO3  per 
t  °.                ioo  Gms. 

G.  Mols. 
CsN03 

Gms.  CsNO3  per 
t  o.                   ioo  Gms. 

G.  Mols  CsNO3 

Solution  . 

Water. 

per  Liter. 

Solution. 

Water'. 

per  loiter. 

O 

8-54 

9-33 

0.476 

60 

45-6 

83.8 

3-41 

10 

12.97 

14.9 

0,725 

70 

51  .7 

107.0 

4.10 

20 

18.7 

23.0 

I  .11 

80 

57-3 

134.0 

4.81 

30 

25-3 

33-9 

1.58 

90 

62  .0 

163  .O 

5-50 

40 

32.1 

47-2 

2.12 

IOO 

66-3 

197.0 

6.19 

50 

39-2 

64.4 

2-73 

106 

.2  68.8 

220-3 

6.58 

CAESIUM    OXALATE 


CAESIUM    OXALATE    Cs2C2O4.H2O. 

SOLUBILITY  OF  MIXTURES  OF  CAESIUM  OXALATE  AND  OXALIC  ACID  IN 

WATER  AT  25°. 

(Foote  and  Andrew  —  Am.  Ch.  J.  34    156,  '05.) 

Varying  amounts  of  the  two  substances  were  dissolved  in  hot  water 
and  the  solutions  allowed  to  cool  in  a  thermostadt  held  at  25°. 


Solid 
Phase. 

H2C2O4.2H2O 

H2C204.2H90  +  H3Cs(C204)2.2H20 

Double  Salt 

H3Cs(C204)2.2H20 

H3Cs(C204)22H20  +  H4Cs2(C204)3 

Double  Salt. 

H4Cs2(C204)3 

H4Cs2(C204)3+HCsC204 

Double  Salt. 
HCsC2O4 

HCsC204+H6Cs8(C204)7 
Double  Salt. 
H6Cs8(C204)7 

H6Cs8(C204)7+Cs2C204.H20 
Cs2C204.H20 


Gms.  per  100 

G.  Mols. 

per  100 

Gms. 

Solution. 

G.  Mols 

H20. 

H2C204 

Cs2C204.          H2C204. 

Cs2C2O4. 

10.  2O 

2.274 

10.29 

•    o 

.61        2.314 

0-035 

7  -9Q 

9 

.92        i 

[-924 

O.6l4  ( 

4.11 

25 

.12             I.l62 

1.81     J 

4-32 

27 

•55 

[.279 

2  .06 

4-2-7 

28 

•30 

[  .267 

2.14   { 

4.40 

35 

.90        3 

.476 

3-07   * 

4.82 

40 

.  10 

[  .752 

3  -71 

4-45 

42 

.32      ] 

.672 

4-05  ) 

3-05 

48 

.80 

.268 

5-i6 

i  .04 

68 

.69         0.688 

11.56  J 

0.91 

71 

.24        0.648 

13.06 

0.77 

73 

•45         0.598 

J4-51  ( 

o-75 

74 

.04        0.596 

14-96  * 

0.74 

75 

.20        0.625 

J5-93 

o.o 

75 

.82        o.o 

I5-97 

CAESIUM   PERMANGANATE  CsMnO4. 

100  cc.  sat.  aqueous  solution  contain  0.097  gm.  CsMnO4  at  i' 
gtn.  at  19°,  and  1.25  gms.  at  59°. 


0.23 


(Patterson  —  J.  Am.  Chem.  Soc.  28,  1735,  !o6.) 


CAESIUM   SELENATE   Cs2SeO4. 

100  grams  H2O  dissolve  245  grams  Cs2SeO4  at  12°. 


(Tutton  —  J.  Chem.  Soc.  71,  850,  '97.) 


CAESIUM    SULPHATE    Cs2SO4. 

SOLUBILITY  IN  WATER. 

(Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203  A,  210,  '04.) 


Gms.  Cs2SO4  per 
to.                  100  Gms. 

G.  Mols. 
Cs2S04 

Solution. 

Water.   • 

per  Liter. 

O 

62.6 

167  .1 

3-42 

IO 

63-4 

I73-I 

3-49 

20 

64.1 

178.7 

3-56 

30 

64.8 

184.1 

3  -62 

40 

65-5 

189.9 

3.68 

50 

66.1 

194.9 

3-73 

Gms.  Cs2SO4  per 
t«.                100  Gms. 

G.  Mols. 
Cs2S04 

Solution. 

Water. 

per  Liter. 

60 

66 

•7 

199 

9 

3 

.78 

7° 

67 

.2 

205 

.0 

3 

•83 

80 

67 

.8 

210 

•3 

3 

.88 

9° 

68 

.3 

214 

9 

3 

.92 

100 

68 

.8 

2  2O 

•3 

3 

•97 

108.6 

69 

.2 

224 

•5 

4 

.00 

CAESIUM    DOUBLE  84 

SULPHATES 

SOLUBILITY  OF  CAESIUM  DOUBLE  SULPHATES  IN  WATER  AT  25°. 

(Locke  —  Am.  Ch.  J.  27,  459,  '01.) 

Cms.  Anhydrous  Salt  Gm.  Mols. 

Name.                                        Formula.                             per  100  Gms.  Salt  per  100 

Solution.       Water.  Gms.H2O. 

Caesium  Cadmium  Sulphate     Cs2cd(SO4)2.6H2o           58.16     139.9  0.2455 

Caesium  Cobalt  Sulphate          Cs2Co(so4)2.6H2o           29.52       41.9  0.081 

Caesium  Copper  Sulphate         Cs,Cu(SO4)2.6H2o          31-49      46.0  0.0882 

Caesium  Iron  Sulphate              Cs2Fe(so4)2.6H2o            50.29     101.1  0.1967 

Caesium  Magnesium  Sulphate  Cs2Mg(so4)2.6H2o          34-77       53-3  0.1106 

Caesium  Manganese  Sulphate  Cs2Mn(so4)2.6H2o          44.58      80.4  0.157 

Caesium  Nickel  Sulphate          Cs2Ni(so4)2.6H2o           20.37       25.6  0.0495 

Caesium  Zinc  Sulphate              Cs2Zn(so4)2.6H2o           27.87      38.6  0.0738 

CAFFEINE    C6H(CH3)3N4O2.H2O. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P. ;  Gockel  —  J.  Chem.  Soc.  74.  327,  '98;  Commaille  —  Compt.  rend.  81,  819,  '75.) 
Grams  Caffeine  per  100  Grams  Solvent  at: 


Solvent. 

25°. 

80°. 

18°. 

b.pt. 

17° 

b.  Dt.      ^ 

U.S. 

P. 

Gockel. 

Commaille. 

Water 

2 

.19 

I9 

23 

. 

,  .  . 

I. 

3it 

45-54 

Alcohol 

I 

.88 

f 

.85* 

. 

.  . 

,  .  . 

o. 

6il§ 

Ether 

O 

.267 

O 

.119 

O 

•295 

o. 

c-44  J§ 

O.^6J§ 

Chloroform 

12 

•5 

. 

II 

•77 

15 

•63 

12  . 

97t 

19.02! 

Benzene 

. 

. 

0 

.911 

5 

.29 

. 

Carbon  Tetra 

Chloride 

. 

.  . 

, 

.  . 

o 

.089 

o 

.702 

. 

Carbon  Bisulphide 

. 

. 

0.0585! 

o-454t 

*  60°.         t  6S°. 

t  Gms 

.  anhydrous  caffeine. 

§ 

Abs.  alcohol  and  abs. 

ether. 

CALCIUM    ACETATE    Ca(CH3COO)2.2H2O. 

SOLUBILITY  IN  WATER. 

(Lumsden  —  J.  Chem.  Soc.  81,  355,  '02;  Krasnicki  —  Monatsh.  Chem.  8,  597,  '87.) 

Gms.  Ca(CH3COO)2  Gms.  Ca(CH3COO)2 

t°.        per  TOO  Gms.                 Solid  Phase.  t°.        per  100  Gms.               Solid  Phase. 

Solution.      \Vater.  Solution.     Water. 

O      27.2      37.4     Ca(CH3COO)2.2H20  60      24.6      32.7  Ca(CH3COO)2.2H2O 

10      26.5      36-0     Ca(CH3COO)2.2H2O  80      25.!      33.5  Ca(CH3COO)2.2H2O 

20      25.8      34.7     Ca(CH3COO)2.2H2O  84  25.3      33.8  Ca(CH3COO)2.2H2O 

25       25 '5      34 -2     Ca(CH3COO)2.2H2O  85  24.7      32.9  Ca(CH3COO)2.H2O 

3°      25-3      33-8     Ca(CH3COO)2.2H20  90  23.7      31.1  Ca(CH3COO)2.H20 

40      24.9      33.2     Ca(CH3COO)2.2H20  IOO  22.9      29.7  Ca(CH3COO)2.H2O 


SOLUBILITY  OF  CALCIUM  ACETATE  IN  AN  AQUEOUS  SATURATED  SOLU- 
TION OF  SUGAR  AT  31.25°. 

(Kohler  — Z.  Ver.  Zuckerind.  47,  447,  *97.) 

TOO  gms.  solution  contain  8.29  gms.  Ca(CH3COO)2  +  60.12  gms.  sugar, 
loo  gms.  water  dissolve  26.3  gms.  Ca(CH3COO)2+  190.3  gms  sugar. 


85  CALCIUM    ACETATES 

CALCIUM    (Tri)    Methyl    ACETATE    Ca[(CH3)3CCOO]a. 
CALCIUM    (Di)    Ethyl    ACETATE    Ca[(C2H6)2CHCOO]2. 
CALCIUM    Methyl    Ethyl    ACETATE    Ca[CH3(C2H6).CHCOO]2. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Landau  —  Monatsh.  Chem.  14,  717,  '93;  Keppish  —  Ibid,  g,  600,  '88;  Sedlitzki  —  Ibid.  8,  573,  '87.> 


Ca.  Tri  Methyl  Acetate. 

Ca.  Di  Ethyl  Acetate.      Ca.  Methyl  Ethyl. 
Acetate. 

Gms.  Ca(C5H9O2)2 

Gms. 

Ca(CeHiiO2)2               Gms.  Ca(C5HfiO2)2 

t  °. 

per  100  Gms. 

per 

100  Gms. 

per 

ioo    Gms. 

Water.     Solution. 

Water 

.     Solution. 

Water. 

Solution. 

0 

7.30     6.81 

30-3 

23.22 

28.78 

22-35 

10 

6.84    6.40 

27.8 

31  .71 

24.07 

20 

6.54     6.14 

25.6 

20.38 

33-76 

25-23 

30 

6.40     6.01 

23-7 

19.16 

34-92 

25.89 

40 

6  .  44     6  .  05 

22  .1 

I8.IO 

35-20 

26-04 

50 

6.64     6.22 

20.8 

17.22 

34.60 

25  .71 

60 

6.86     6.42 

19-9 

16.60 

33-n 

24.89 

70 

7.11     6  .  64 

19.2 

16.11 

30-74 

23.41 

80 

7.38     6.87 

27.49 

21  .56 

CALCIUM    Methyl    Propyl    ACETATE     Ca[CH3(C3H7).CHCOO]:. 
CALCIUM    (Di)    Propyl    ACETATE    Ca[(C3H7)2CHCOO]2. 
CALCIUM    (Iso)    Butyl    ACETATE    Ca[(CH3)2CH(CH2)2COO]2. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Stiassny  —  Monatsh.  Chem.  12,  596,  '91;  Furth  —  Ibid.  9,  313,  '88;  Konig  —  Ibid.  15,  22,  '94.) 

Ca.  Methyl  Propyl  Acetate.     Ca.  Di  Propyl  Acetate.     Ca.  Iso  Butyl 

Acetate. 

Gms.  Ca(C6HnO2)2  Gms.  Ca(C8H15O2)2  Gms.  Ca(C6HuO2)2 

t  o^  per  ioo  Gms.  per  ioo  Gms.  per  ioo  Gms. 

Water.     Solution.  Water.     Solution.  Water.     Solution. 

o  16.58  14.22  9.57  8.73  7.48  6.96 

10  15.80  13.65  8.35  7.71  6.38  5.99 

20  15-14  I3-I5  7-I9  6.71  5-66  5-36 

30  14.61  12.75  6-I3:  5-77  5-31  5-04 

40  14.21  12.45  5-°9  4-84  5-31  5-°4 

50  13.94  12.24  4-i4  3-98  5-68  5-37 

60  13-79  12.13  3-25  3-15  6-4i  6.02 

70  13.78  12.12  2.44  2.38  7.51  6.98 

80     13-89   12.20          1-65   1.62         8.97   8.23 

90  10.79  9-74 

CALCIUM    BROMIDE    CaBr2. 

SOLUBILITY  IN  WATER. 


(Kremers  —  Pogg 
yield  £ 

—  22 
O 
10 
20 
25 

;.  Ann.  103,  65,  '58;  Etard  —  ^ 
in  irregular  curve  and  are  evid< 

ims.  CaBr2  per  ioo  Gms. 

\nn.  chim.  phys.  [ 
;ntly  less  accurate 

34-2 
40 
60 
80 

?!  2,  532,  *94.  gives  results  which 
than  those  of  Kremers.) 

tns.  CaBr2  per  ioo  Gms. 

Water. 
101 

I25 

I32 
153 

Solution. 
50-5 

55-5 
57-o 
58.8 
60.5 

Water. 

213 
278 

295 
312 

Solution. 
65 

68.1 
73-5 
74-7 
75-7 

Density  of  saturated  solution  at  20°  =  1.82. 


CALCIUM    BUTYRATE 


86 


CALCIUM    (Normal)    BUTYRATE    Ca[CH3(CH2)2COO]2.H2O. 

CALCIUM    (Iso)    BUTYRATE    Ca[(CH3)2CH.COO]2.sH2O. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Lumsden  —  J.  Chem.  Soc.  81,  355,  '02;  see  also  Chancel  and  Parmentier  —  Com pt.  rend.  104,  474, 
'87;  Deszathy  —  Monatsh.  Chem.  14,  251,  '93,  and  also  Hecht  —  Liebig's  Annalen  213,  72,  '82,  give 
results  for  the  normal  salt  which  are  somewhat  below  those  of  Lumsden  for  the  lower  temperatures. 
SedJitzki  —  Monatsh.  Chem.  8,  566,  '87,  gives  slightly  different  results  for  the  iso  salt.) 

Calcium  Iso  Butyrate. 


Calcium  Normal  Butyrate. 

Gms.  Ca(C4H7O2)2 

t  ° 

per  ] 

too  Gms. 

t°. 

Water. 

Solution. 

0 

20.31 

16.89 

o 

10 

J9-i5 

16.08     ' 

20 

20 

18.20 

J5-39 

30 

25 

17.72 

!5-°5 

40 

30 

17.25 

14.71 

60 

40 

16.40 

14.09 

62 

60 

15.15 

13.16 

65 

80 

14-95 

13  .01 

80 

100 

15-85 

13.69 

100 

Gms.  Ca(C4H702)2 
per  100  Gms. 

Water.      Solution. 


Solid 
Phase. 


20 .10  16 . 78  Ca(C4H702)2.5H20 

22.40  18.30 

23.80  19.23 

25.28  20.65 

28.40  22.12 

28.70  22.30 

28.25  22.O3 

27.00  21.26 

26.IO  20.69 


CALCIUM    CAPROATE    Ca[CH3(CH2)4COO]2.H2O. 

CALCIUM     3     Methyl     PENTANATE       Ca[CH3.CH2.CH(CH3)CH2. 
COO]2.3H20. 

CALCIUM    CAPRYLATE    Ca[CH3(CH2)6COO]2.H2O. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Lumsden;  the  Pentanate,  Kulish  —  Monatsh.  Chem.  14,  566,  '93;  see  also  Keppish  —  Ibid,  g,  594, 
'88,  and  Altschul  —  Ibid.  17,  571,  '96,  for  results  on  the  Caproate.) 

Ca.  Caproate. 


Gms.  Ca(CaHuOa)2 
t    .        per  100  Gms. 
H20. 

O 
20 

2.23 
2.18 

40 

2.15 

50 
60 
80 

2  .IO 
2.15 
2.30 

100 

2-57 

Ca. 

3  Methyl  Pentanate. 

Ca.  Caprylate. 

Gms.  Ca(C6HnO2)2 
per  100  Gms, 

Gms.  Ca(C8H15O2)s 
per  zoo  Gms. 
H20. 

o-33 

0.31 
0.28 
O.26 

Water.       Solution. 

12.33     IO-98 

I7.l8       14.66 

18.99     *5-97 
18.73     I5-78 

17.71     15.04 
13.37     ii  -80 

0.24 
0.32 

9-94      9-04 

0.50 

CALCIUM    CARBONATE    CaCO3. 

SOLUBILITY  IN  WATER,  AS  DETERMINED  BY  THE  ELECTROLYTIC 
CONDUCTIVITY  METHOD. 

(Holleman,  Kohlrausch,  and  Rose  —  Z.  physik.  Chem.  12,  129,  241,  '93.) 

i  liter  solution  contains  o.oi  gram  CaCO3  at  8.7°,  and  0.012  gram 
at  20°. 


87    CALCIUM  BICARBONATE 

CALCIUM  BICARBONATE  Ca(HCO3)2. 

SOLUBILITY  IN  WATER  AT  15°. 

Calcium  carbonate  in  presence  of  water,  free  from  and  containing 
carbon  dioxide,  dissolves  as  the  hydrogen  carbonate. 

(Among  the  investigators  who  have  reported  results  upon  the  solubility  of  calcium  bicarbonate  may  be 
mentioned,  Cossa  —  Z.  anal.  Chem.  8,  145,  '69;  Schloesing  —  Com pt.  rend.  74,  1522,  '72;  Caro  —  Arch. 
Pharm.  [3]  4,  145,  '74;  Reid  —  Proc.  Roy.  Soc.  (Edin.)  15,  151,  '87-'88;  Irving  and  Young  —  J.  Chem. 
Soc.  56,  344,  '88;  Anderson  —  Proc.  Roy.  Soc.  (Edin.)  16,  319,  '88- '89  ;  Engel  —  Ann.  chim.  phys. 
[6]  I3>  348,  '88;  Lubavin  —  J.  russ.  phys.  chem.  Ges.  24,  389,  '92;  Pollacci  —  L'Orosi  19,  217,  '96, 
etc.  The  results,  however,  which  appear  of  most  interest  and  reliability  are  the  following  by  Tread- 
well  and  Reuter  —  Z.  anorg.  Chem.  67,  185,  '96.) 

cc.  CC»2  per  100  cc.         Partial  Pres-  Gms.  per  100  cc.  Saturated  Solution. 

Gaseous  Phase  sure  of  CC>2 

(o°  and  760  mm.).          in  mm.  Hg. 

8.94  67.9 

6.04  45-9 

5-45  4i-4 

2.18  16.6 

1.89  14.4 

1.72  13.1 

0.79  6.0 

0.41  3-1 

0.25  1.9 

o . 08  o • 6 


Therefore  i  liter  sat.  solution  at  15°  and  o  partial  pressure  of  CO2 
contains  0.385  gram  Ca(HCO3)2. 


SOLUBILITY  OF  CALCIUM  BICARBONATE  IN  AQUEOUS  SODIUM  CHLORIDE 

SOLUTION  AT  15°. 

(Tread well  and  Reuter.) 

The  NaCl  solution  contained  about  5  grams  per  liter,  and  was  there- 
fore approximately  TV  normal. 

cc.  CC>2  per  I0°  cc.       Partial  Pres-  Grams  per  100  cc.  Saturated  Solution. 

(1  aseous  Phase  sure  of  CO2 

(o°  and  760  mm.).          in  mm.  Hg. 

16.95          I28'8 

11.47       87-2 

6.07  46.1 

3.16  24.0 

0.50  3-8 

•4i        3-4 


Free  CO2. 

Ca(HC03)2. 

Ca. 

0.1574 

0.1872 

0.0462 

0-0863 

0-1755 

0-0433 

0.0528 

0-1597 

0.0394 

0.0485 

O.I54O 

0-0380 

0.0347 

O.I492 

0.0368 

0-0243 

Q-I331 

0.0329 

O.OI45 

0.1249 

0.0308 

o  .  0047 

0.0821 

O.O2O3 

O.OO29 

0-0595 

O.OI47 

0.0402 

0.0099 

0.0385 

0.0095 

Free  CO2. 

Ca(HC03)2. 

Ca. 

0.1325 

0.2184 

0-0539 

O-IIOI 
0.0235 
0.0135 

0.0027 

0.2143 
0.1492 
0-1183 
0-0739 

0-0529 
0.0368 
0.0292 
O.Ol82 

0.0003 

o  .  0490 

0-0349 
0.0332 

O.OI2I 
0.0086 
0.0082 

CALCIUM    BICARBONATE 


88 


SOLUBILITY  OF  CALCIUM   BICARBONATE   IN  AQUEOUS   SOLUTIONS  OT 
AMMONIUM  NITRATE,  SODIUM  CHLORIDE  AND  OF  SODIUM  SULPHATE. 

(Cameron  and  Seidell  —  J.  Physic.  Chem.  6,  50,  '02;  Berju  and  Kosminiko  —  Landw.  Vers.  Stat.  60, 

422,  '04.) 


In  NI^NOa  Solutions  at  18°.      In  NaCl  Solutions  at  25°. 
Grams  per  Liter  Solution.        Grams  per  Liter  Solution. 


In  Na2SO4  Solutions  at  24° 
Grams  per  Liter  Solution. 


rH4NO8 

.    Ca(HC03)2. 

NaCl. 

Ca(HC03)2. 

Na2S04. 

Ca(HCO3)2  total. 

Ca(HC03)2. 

o 

O.2IO 

0 

o  .  1046 

O 

0.092 

0.092 

5 

10 
20 

0.340 
0.415 

0-547 

5 

10 

20 

0.150 
O.lSo 
O.2IO 

5 

IO 
20 

0-175 
0.232 

0.277 

0.22O 
O.262 

40 
80 

0.744 
0.940 

40 
80 

O.225 
O.22O 

40 
80 

o-332 
0.400 

0.307 

o-347 

IOO 

150 

2OO 

0.215 
0.192 
0.170 

IOO 
200 

0.432 
0.510 
0.600 

o-355 
0.382 
0.400 

250 

0.137 

250 

0.725 

o-435 

CALCIUM    CHLORATE    Ca(ClO3)2.2H2O. 

100  grains  saturated  aqueous  solution  contain  64.0  grams  Ca(ClO3X 
at  1 8°.     Density  of  solution  is  1.729. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 


CALCIUM    CHLORIDE    CaCl2. 

SOLUBILITY   IN   WATER. 

(Roozeboom  —  Z.  physik.  Chem.  4,  42,  '80;  see  also  Mulder;  Ditte  — 
—  Ann.  chim.  physic.  [6Ji3,  381,  '88;  Etard  —  Ibid 


Com pt.  rend.  92,  242,  '81;  Eng"* 
•  [?]  2,  532,  '94.) 


Gms.  CaCl2  per 
100  Gms. 


Solid 
Phase. 


Water.  Solution. 

29.8    Ice  +  CaCl2.6H2O 
33.3    CaCl2.6H2O 

37.3  CaCl2.6H2O 

39.4  CaCl2.6H2O 
42  . 7    CaCl2.6H2O 
50.7    CaCl2.6H2O 
47  . 6    CaCl2.4H2Oa 
50.1    .4H2Oa+.6H2O 
53-4    -4H2Oa 

5I.I    CaCl2.4H2OB 
53  .O    .<iH2O  8  +  .6H2O 

55  .o  ^H2o  8 

56.0    ^H2O/3+CaCl2.2H2O 
56.6    wtHjsO  a  +  CaCl2.2H2O 

Density  of  saturated  solution  ato°=  1.367,  at  15°=  *-399»  at  18° 
—  1.417. 


-55 

42-5 

-25 

50.0 

O 
10 

59-5 
65.0 

20 

74-5 

30.2 

102.7 

2O 
29.8 

91  .0 
ioo.  6 

40 

I][5-3 

20 

104.5 

29.2 

112.  8 

35 

122.5 

38-4 

127-5 

45-3 

130.2 

Gms.  CaCl2  per 
t°.                   loo  Gms. 

Solid 

•DV.r.00 

Water.    Solution.     *"a~" 

60 

136 

,8 

57-8 

CaCl2.2H2O 

70 

141. 

7 

58.6 

CaCl2.2H2O 

80 

147 

.0 

59-5 

CaCl2.2H2O 

90 

J52 

•7 

60.6 

CaCl2.2H2O 

IOO 

.0 

61  .4 

CaCl2.2H20 

120 

I73 

.0 

63-4 

CaCl2.2H2O 

140 

191 

.0 

65.6 

CaCl2.2H2O 

160 

222 

•5 

69.0 

CaCl2.2H2O 

170 

255 

•  0 

71.8 

CaCl2.2H2O 

r75-5 

297 

.0 

74-8J 

CaCl2.2H2O 
-f  CaCl2.ii2O 

180 

300 

.0 

75-o 

CaCl2H2O 

200 

311 

•  0 

75-7 

CaCl2.H20 

235 

332 

.0 

76.8 

CaCl2.H2O 

260 

347 

.0 

77.6 

CaCl2.H2O 

89 


CALCIUM    OHLORIDE 


SOLUBILITY  OF  CALCIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROCHLORIC  ACID  AT  o°. 

(Engel  —  Compt.  rend.  104,  434,  '87.) 


G.  Mols.  in  Mgs. 
per  10  cc. 

Solution. 

HCL 
O.O 


92.7 

83-7 

77.1 

66.25 

53-75 
36-25 
20.3 


16.0 

29.25 

43-45 

63-5 

95-o 


Density  of 
Solutions. 

.367 

•344 
.326 
.310 
.283 
.250 
-238 


Grams  per  ioo  cc. 
Solution. 

CaCl2. 

HCl. 
O.O 

46.45 
42.80 

36-77 
29.84 

3-32 
5-83 

10.66 
15.84 

2O.  1  2 
II  .29 

23  •I5 
34.62 

SOLUBILITY  OF  MIXTURES  OF  CALCIUM  CHLORIDE  AND  ALKALI 

CHLORIDES. 

(Mulder;  Rudorff.) 

ioo  grams  H2O  dissolve  63.5  grams  CaCl2  +4-9  grams  KC1  at  7°  (M) 
100  grams  H2O  dissolve  57.6  grams  CaCl2  +  2.4  grams  NaCl  at  4°  (M) 
ioo  grams  H2O  dissolve  59.5  grams  CaCl2 +4.6  grams  NaCl  at  7°(M) 
ioo  grams  H2O  dissolve  72.6  grams  CaCl2  + 16.0  grams  NaCl  at  i5°(R) 


SOLUBILITY  OF  CALCIUM  CHLORIDE  IN  AQUEOUS  ALCOHOL  AT  ROOM 

TEMPERATURE. 

(Bodtker  —  Z.  physik.  Chem.  22,  570,  '97.) 


Solution 
Used. 

15  Cms.  CaCl2.6H2O 

+  20  cc.  alcohol 
15  Gms.  CaCl2.6H2O 

+  20  cc.  alcohol 
15  Gms.  CaCl2.6H2O 

+  20  cc.  alcohol 
15  Gms.  CaCl2.6H2O 

+  i  Gm.  CaCl2 


Vol. 

per 

cent 

Alcohol. 


92-3 


97-3 


99-3 
99-3 


Gms. 
CaCl2 


1.430 


1.409 


1.429 


1.529 


Solution 
Used. 


15  Gms.  CaCl2.6H2O-f  2occ. 
alcohol  +  2  Gms.  CaCl2 

"  +3  "  " 
«  +4  «  « 
„  +5  "  " 


Vol.       Gms. 
per        CaCl2 
cent     per  5  cc. 
Alcohol.      Sol. 


99-3 


1.561 
1.590 
1 .641 
1.709 


SOLUBILITY   OF   CALCIUM   CHLORIDE   IN   A   SATURATED  SOLUTION  OF 

SUGAR  AT  31.25°. 

(Kohler  — Z.  Ver.  Zuckerind.  47,  447,  '97-) 

ioo  grams  saturated  solution  contain  42.84  grams  sugar  +  25.25 
grams  CaCl2,  or  ioo  grams  water  dissolve  135.1  grams  sugar  +  79.9 
grams  CaCl2. 


CALCIUM    CITRATE    Ca3(C6H5O7)2.4H2O. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL  AT  18°  AND  AT  25* 

(Partheil  and  Hiibner  —  Archiv.  Pharm.  241,  413,  '03-) 


Solvent. 


Grams  Caa 
per  ioo  Gms.  Solvent  at: 


Water  0.08496        0.0959 

Alcohol  (Sp.  Gr.  0.8092  =  95%)         0-0065          0.0089 


CALCIUM    CHROMATE 


90 


CALCIUM    CHROMATE    CaCrO4. 

SOLUBILITY  OF  THE  SEVERAL  HYDRATES  IN  WATER. 

(Mylius  and  Wrochem  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  462,  'oo.) 


Gms.CaCr04penooGms.  Mols-  CaC/°* 


Water. 

Solution.         H20. 

Solid  Phase, 

CaCr044H2O 

7-3 

6.8 

0.84 

4-8 

4-4 

0.51 

3  -84 

3-7 

0.44 

5 

2.67 

2.6 

0.31 

1-63 

1.6 

0.19 

i-i3 

1  .1 

0.13 

0.81 

0.8 

0.09 

Solid  Phase,  CaCrO4. 

4-5 

4-3 

0.52 

2.32 

2.27 

0.27 

2.92 

1.89 

O.22 

1.  12 

i  .11 

0.13 

0.83 

0.82 

O-II 

0.80 

0.79 

O.O9 

0.42 

0.42 

O.O5 

1 0  Cms.  CaCrO4  per  100  Cms.    Mols.CaCrO4 
*   •     • — TTT- " — ~  .     . >  per  100  Mols. 


O 

18 

31 
38 
50 
60 
100 

o 
18 

3i 
50 
60 

70 

100 


Densities  of  the  saturated  solutions  of  the  above  several  hydrates 
at  18°  are:  a  CaCrO4.2H2O,  1.149;  ft  CaCrO4.2H2O,  1.105;  CaCrO4.H2O, 
1.096;  CaCrO4.iH2O,  1.044;  CaCrO4,  1.023. 

100  cc.  29%  alcohol  dissolve  1.206  grams  CaCrO4. 
100  cc.  53%  alcohol  dissolve  0.88  gram  CaCrO4. 

(Fresenius  —  Z.  anal.  Chem.  30,  672,  '91.) 


CALCIUM    POTASSIUM    FERROCYANIDE    CaK2Fe(CN)6.3H2O. 
100  parts  H2O  dissolve  0.125  part  salt  at  15°,  and  0.69  part  at  b.  pt. 

(Kunheim  and  Zimmerman  —  Dingt.  polyt.  J.  252,  478,  '84.) 

CALCIUM    FLUORIDE    CaF2. 

i  liter  of  saturated  aqueous  solution  contains  0.016  gram  CaF2  at 
1 8°.     Determined  by  the  electrolytic  method. 

(Kohlrausch  —  Z.  physik.  Chem.  44,  197,  '03.) 


Water.             Solution. 

UC1     imj    -i.Vl.LMa. 

H20. 

Solid  Phase,  a  CaCrO4.2H2O. 

(Monoclinic.) 

O 

17-3          J4-75 

2  .O 

18 

16.68         14.3 

1.93 

20 

16.6          14.22 

I  .93 

30 

16.5           13.89 

1.85 

45 

14-3           I2-53 

1.65 

Solid 

Phase,  ft  CaCrO4.2H20  (Rhombic.) 

0 

10.9            9.8 

1-25 

18 

11.5           10.3 

40 

n.  6          10.4 

i-34 

Solid  Phase,  CaCrO4.H2O 

0 

13.0              II-5 

1.50 

18 

10.6            9.6 

I  .22 

25 

10.  o            9.1 

I  .15 

40 

8-5            7-8 

0.98 

60 

6.1            5.7 

0.70 

75 

4.8            4.6 

0.56 

100 

1    2                  ^  .1 

O                               O 

o-37 

CALCIUM    FORMATE    Ca(HCOO)2. 

SOLUBILITY  IN  WATER. 

(Lumsden  —  J.  Chem.  Soc.  81,  355,  '02;  see  also  Krasnicki  —  Monatsh.  Chem.  8,  597,  '87.) 


Gms.Ca(HCOO)2 
t°.                  per  100  Gms.                             4° 

Gms.Ca(HCOO)2 
per  TOO  Gms. 

O 
20 

40 

Water. 
16.15 

16.60 
I7-05 

Solution. 
13.90 
14.22 
14.56 

60 
80 
100 

Water. 
17.50 

17-95 
18.40 

Solution. 
14-89 
15  .22 
15-53 

9i  CALCIUM    HEPTOATE 

CALCIUM    HEPTOATE    (Oenanthate)    Ca[CH3(CH2)6COO]2.H2O. 

SOLUBILITY  IN  WATER. 

(Lumsden  —  J.  Chem.  Soc.  81,  355,  '02;  see  also  Landau  —  Monatsh.  Chem.  14,  712,  '03;  Altschul  — 

Ibid.  17,  575,  '96.) 

t°.  o°.  20°.  40°.  60°.  80°.         100°. 

G.  Ca(C7H1302)2  per 

100  gms.  solution        0.94    0.85     0.81     0.81     0.97     1.24 

CALCIUM    HYDROXIDE    Ca(OH)?. 

SOLUBILITY  IN  WATER, 

(Average  curve  from  the  results  of  Lamy  —  Ann.  chim.  phys.  [5]  14,  145,  '78;  Mahen  —  Pharm.  J.  Trans 
[3]  14.  5°5,  '83-84;  Herzfeld  —  Z.  Ver  Zuckerind.  34,  820,  '97,  and  Guthrie  —  J.  Soc.  Chem.  Ind.  20, 
224,  *oi.) 

0  Grams  per  100  Grams  H2O.  Grams,  per  TOO  Grams  H2O. 

Ca(OH)2.  CaO.  Ca(OH)2.  CaO.  " 

o  0.185  0.140  50  0.128  0.097 
10  0.176  0.133  60  0.116  0.088 
20  0.165  0.125  70  0.106  0.080 

25       0.159      0.120  80       0.094      0.071 

30  0.153  0.116  90  0.085  0.064 

40  0.141          o«.  107  100  0.077          0.058 


SOLUBILITY    QF    CALCIUM    HYDROXIDE    IN    AQUEOUS  SOLUTIONS    OP 
AMMONIUM  CHLORIDE  AT  25°. 

(Noyes  and  Chapin  —  Z.  physik.  Chem.  28,  520,  'oo.) 

Millimols  per  Liter.  Grams  per  Liter  of  Saturated  Solution. 

NEUCl Ca(OH)2.  NtUCl c£(OH)2  =  CaO. 

o.oo        20.22  o.oo          1-50  1.13 

21.76  29.08  I-l65  2.l6  1.63 

43.52        39 .23  2-33°        2.91  2 -20 

83-°7         59 -68  4-447        4-42  3-45 


SOLUBILITY    OF    CALCIUM    HYDROXIDE    IN    AQUEOUS    SOLUTIONS    OF 

CALCIUM  CHLORIDE. 

(Zahorsky  —  Z.  anorg.  Chem.  3,  41,  '93;  Lunge  —  J.  Soc.  Chem.  Ind.  u,  882,  '92.) 

Concentration  Grams  CaO  Dissolved  per  100  cc.  Solvent  at: 

ofCaCl2Solutions,Wt.%.         -—      ~^~        ~£T  ^ ~^ 

o  0.1374  0.1162  0.1026  0.0845  0.0664 

5  0.1370  0.1160  0.1020  0.0936  0.0906 

10  0.1661  0.1419  0.1313  0.1328  0.1389 

15  0.1993  0.1781  0.1706  0.1736  0.1842 

20         0.1857*   0.2249    0.2204   0.2295   0.2325 

25       0.1661*  0.3020*  0.2989  0.3261  0.3710 
30       0.1630*  0.3680*  0-3664  0.4122  0.4922 

*  Indicates  cases  in  which  a  precipitate  of  calcium  oxychloride 
separated  and  thus  removed  some  of  the  CaCl2  from  solution.  ^ 

The  results  in  o%  CaCl2  solutions,  i.e.,  in  pure  water,  are  high  when 
compared  with  the  average  results  given  above. 


CALCIUM    HYDROXIDE 


92 


SOLUBILITY   OF   CALCIUM    HYDROXIDE   IN   AQUEOUS   SOLUTIONS   OP 
POTASSIUM  CHLORIDE  AND  OF  SODIUM  CHLORIDE. 

(Cabot  — J.  Soc.  Chem.  Ind.  16,  417,  '97.) 


Cms.  of  the 
Chloride 
per  Liter. 

O 

30 
60 
1  2O 
240 
320 

In  KC1  Solutions.                           In  NaCl  Solutions. 

Gms.  CaO  per  Liter  at:                                     Cms.  CaO  per  Liter  at: 

b°. 

1.36 

I.70I 

I-725 
I.7l8 
1.248 

15°. 

I-3I 
1.658 
1.674 
I.  606 
I.IQ9 

99&. 

o-635 

0.788 
0.876 

0.894 
0.617 

o°. 

•36 
.813 

.86 

•37 
•054 

15°. 

i-3i 
1.703 
1.824 
i  .722 
1.274 
0.929 

99°. 

°-635 
0.969 
1  .004 
1  .015 

0.771 

0.583 

SOLUBILITY  OF  LIME  IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE 

ALONE    AND    CONTAINING   SODIUM    HYDROXIDE. 
(Margiet  —  Bull.  soc.  chim.  [3]  33,  631,  '05.) 


Gms.  CaO  per  Liter  of  Solution. 

per  liter.  Without    0.89  .NaOH    4  .09  .NaOH 
NaOH.      per  Liter.        per  Liter. 

O.22 


0 

J-3          < 

5.8 

5 

1.4       < 

3.9 

10 

1.6 

.0 

25 

i-7 

.1 

50 

1.8 

•25 

75 

i  .9 

•4 

100 

1.85 

•4 

G.  NaCl. 
per  Liter. 

150 

182 
225 
250 
300 


Gms.  CaO  per  Liter  of  Solution. 


Without 
NaOH. 


o.89.NaOH     4.o9.NapH 
per  Liter.        per  Liter. 


I  .2 
I  .2 
I  .0 

0.9 

0-7 


0-44 


O.22 


SOLUBILITY    OF    CALCIUM    HYDROXIDE    IN    AQUEOUS    SOLUTIONS  OF 
SODIUM   HYDROXIDE. 

(d'Anselme  —  Bull.  soc.  chim.  [3]  29,  938,  '03.) 


Concentration  of  NaOH: 


Grams  CaO  per  Liter  Sat.  Solution  at: 


Normality. 

Gms.  per  Liter 

O 

O 

N/ioo 

0-4 

N/25 

1.6 

N/is 

2.66 

N/8 

5-00 

N/5 

8.00 

N/2 

20-00 

To°. 

50°. 

70°. 

100°. 

i  .  170 
0.94 

0.880 
0.65 

o-75 
o-53 

o-54 
o-35 

o-57 

o-35 

0.225 

0.14 

o-39 
0.18 

O-2O 
0.06 

O.II 

0.04 

0.05 
o.oi 

O.II 

O-O2 

O-OI 

trace 

0.02 

trace 

o.oo 

o.oo 

For  results  upon  mixtures  of  calcium  hydroxide  and  alkali  carbonates 
and  hydroxides,  see  Bodlander  —  Z.  angew.  Chem.  18,  1138,  '05. 


93  CALCIUM    HYDROXIDE 

SOLUBILITY    OF    CALCIUM    HYDROXIDE    IN    AQUEOUS    SOLUTIONS    OP 

GLYCERINE  AT  25°. 


(Herz  andKnoch  —  Z.  anorg.  Chem.  46,  193,  '05;  for  older  determinations,  see  Berthelot  —  Ann.  chim. 
phys.  [3]  46,  176;  and  Carles  —  Arch.  Pharm.  [3]  4,  558,  '74.) 

Density  of 
Solutions 

Wt.  per  cent 
Glycerine 
in  Solution. 

Millimols 
*Ca(OH)2  per 
100  cc.  Solution. 

Gms.  per 

100  cc.  Solution. 

Ca(OH)2 

=       CaO/ 

1.0003 

o.o 

4-3 

0-1593 

o.i  206 

1.0244 

7-*S 

8.13 

0.3013 

O.228l 

1-0537 

20.44 

14.9 

0.5522 

0.4180 

I  .0842 

3i-55 

22.5 

0-8339 

0.6313 

I.II37 

40.95 

40.1 

1.486 

I.I25 

i  -i356 

48.7 

44-o 

1.631 

1.234 

1.2072 

69.2 

95-8 

3-550 

2.687 

SOLUBILITY  OF  LIME  IN  AQUEOUS  SOLUTIONS  OF  SUGAR. 

(Weisberg  —  Bull.  soc.  chim.  [3]  21,  775,  '99.) 

The  original  results  were  plotted  on  cross-section  paper  and  the 
following  table  constructed  from  the  curves. 

ist  series,  t°  =  i6/-i7°. 


>ms.  p 

Sr  100  Gms. 

Sc 

ution. 

G.  CaO  per  100 

Gms.  Sugar  in  Sol. 

Sugar. 

CaO. 

I 

0.30 

35-o 

2 

0.56 

28.7 

3 

0.85 

28.0 

4 

I  .12 

27.7 

5 

I  .40 

27-5 

6 

1.65 

27-5 

8 

2  .22 

27-5 

10 

2-77 

27-5 

12 

3-27 

27-5 

14 

3-85 

27-5 

2d,  series  t°  = 

=    i  er° 

Gms.  pe 

:r  100  Gms. 

Sc 

lution. 

G.  CaO  per  100 

Sugar. 

CaO. 

VJITIS.  oiigur  in  ool. 

I 

0.50 

62.5 

2 

o-75 

36.0 

3 

i  .02 

32.5 

4 

I  .22 

30.2 

5 

i-45 

28.5 

6 

1.67 

27.7 

8 

2  .22 

27-5 

10 

2-77 

27-5 

12 

3-27 

27-5 

14 

3-85 

27-5 

In  the  second  series  a  very  much  larger  excess  of  lime  was  used  than 
in  the  first  series.  The  author  gives  results  in  a  subsequent  paper,  — 
Bull.  soc.  chim.  [3]  23,  740,  'oo,  — which  show  that  the  solubility  is  also 
affected  by  the  condition  of  the  calcium  compound  used,  i.e.,  whether 
the  oxide,  hydrate,  or  milk  of  lime  is  added  to  the  sugar  solutions. 


CALCIUM    IODATE 


94 


CALCIUM    IODATE    Ca(IO3)2.6H2O. 

SOLUBILITY  IN  WATER. 

(Mylius  and  Funk  —  Ber.  30,  1724,  '97;  W.  Abh.  p.  t.  Reichanstalt  3,  448,  'oo.) 


t  °. 

Gms. 
Ca(I03)2 
per  ioo 
Gms.  Sol. 

Mols. 
Ca(I03)2 
per  ioo 
Mols.H2O. 

Solid 
Phase. 

t°. 

Gms. 
Ca(I03)2 
per  ioo 
Gms.  Sol. 

Mols. 
Ca(I03)2 
per  ioo 
Mols.  H2O. 

Solid 
Phase. 

0 

O 

.10 

0.0044    Ca(IO3)  .611,0      21 

O 

37 

O 

.016  Ca(IO3)2.H2O 

10 

O 

•17 

0.0075 

§f 

35 

O 

.48 

0 

.021 

14 

18 

O 

•25 

O.OII 

« 

40 

0 

•52 

O 

.023 

(I 

30 

O 

.42 

0.019 

tt 

45 

O 

•54 

O 

.024 

11 

40 

O 

.6l 

0.027 

« 

5o 

o 

59 

O 

.026 

(I 

5° 

O 

.89 

0.040 

« 

60 

o 

-65 

0 

.029 

11 

54 

j 

.04 

0.046 

« 

80 

0 

79 

O 

•034 

« 

60 

j 

36 

0.063 

n 

IOO 

0 

94 

O 

.042 

« 

Density  of  solution  saturated  at  18°  =  i.oo. 

CALCIUM    IODIDE    CaI2. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  the  results  of  Kremers  —  Pogg.  Ann.  103,  65,   '58;  Etard  —  Ann.  chim.  phys.  [7] 

2.  532,  '94-) 


O 
10 
2O 


Gms.  CaI2  per  100 
Gms.  Solution. 

64.6 

66.0 
67.6 


30 
40 
60 


Gms.  CaI2  per  100 
Gms.  Solution. 

69 
70.8 

74 


t  °. 

80 
100 


Gms.  CaI2  per  100 
Gms.  Solution. 

78 

81 


Density  of  solution  saturated  at  20°  —  2.125. 

CALCIUM  (Neutral)  MALATE  Ca(C4H4O5).3H2O. 
CALCIUM  (Acid)  MALATE  Ca(C4H5O5)2.6H2O. 
CALCIUM  MALONATE  Ca(C3H2O4).4H2O. 

SOLUBILITY  OF  EACH  IN  WATER. 


(Iwig  and  Hecht  —  Liebig's  Ann.  233,  167,  '86;    Cantoni  and  Basadonna  —  Bull.  soc.  chim.  [3]  35 
731,  '06;  the  malonate,  Miczynski  —  Monatsh.  Chem.  7,  261,  '86.) 

Ca.  Neutral  Malate.                    Ca.  Acid  Malate.     Ca.  Malonate. 

Gms.  Ca(C4H405) 

per  ioo. 

Gms.  Ca(C4H5O5)2 

Gms.  Ca(C3H2O4) 

t  °. 

Gms. 

Gms. 

cc.  Sol. 

per  ioo  Gms. 

per  ioo 

H20. 

Sol. 

(C  and  B). 

Water. 

Solution. 

Gms.  H2O. 

0 

0.290 

10 

0.85 

0.84 

1.8 

1-77 

0-330 

20 

0.82 

0.81 

0.907 

I  .5 

1.48 

o-365 

30 

0.78 

o-77 

0.835 

2.0 

I  .96 

0.396 

40 

0-74 

o-73 

0.816 

5-2 

4-94 

0.422 

50 

0.66 

0.65 

0.809 

15.0 

13.09 

0-443 

57 

o-57 

0.56 

32.24 

24.29 

60 

0.58 

0.58 

0.804 

26.0 

20.64 

0.460 

70 

0.63 

0.63 

0-795 

II  .O 

9.91 

0.472 

80 

0.71 

0.70 

o-754 

6.8 

6-37 

0.479 

90 

0.740 

SOLUBILITY  OF  CALCIUM  MALATE  IN  WATER  AND  IN  ALCOHOL. 

(Partheil  and  Hiibner  —  Archiv.  Pharm.24i,  413,  '03.) 

ioo  grams  H2O  dissolve  0.9214  gram  CaC4H4O5.H2O  at  18°,  and 
0.8552  gram  at  25°. 

ioo  grams  95%  alcohol  dissolve  0.0049  gram  CaC4H4O6.H2O  at  18°, 
and  0.00586  gram  at  25°. 


95  CALCIUM    NITRATE 

CALCIUM    NITRATE    Ca(NO3)2.2H2O. 

SOLUBILITY  IN  WATER  AT   18°. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 

ioo  grams  saturated  solution  contain  54.8  grams  Ca(NO3)2.    Density 
of  solution,  1.548. 

CALCIUM    OXALATE    Ca(COO)2.H2O. 

SOLUBILITY  IN  WATER,  BY  ELECTROLYTIC  CONDUCTIVITY  METHOD. 

(Holleman,  Kohlrausch,  and  Rose  —  Z.  physik.  Chem.  12,  129,  241,  '93;  Richards,  McCaffrey, 
and  Bisbee  —  Z.  anorg.  Chem.  28,  85,  '01.) 

-o  Cms.  CaC2O4  per  to  Cms.  CaC2O4  per 

Liter  of  Solution.  Liter  of  Solution. 

13        0.0067  (H)  25         0.0068  (R,  McC  and  B) 

18        0.0056  (K  and  R)  50        0.0095 

24        0.0080  (H)  95        0.0140  " 


SOLUBILITY  OF  CALCIUM  OXALATE  IN  AQUEOUS  SOLUTIONS  OF  ACETIC 

ACID    AT    26°-27°. 
(Herz  and  Muhs  —  Ber.  36,  3715,  '03.) 

Normality  of  G.  CH3COOH  Residue  from  50.052 

Acetic  Acid.  per  ioo  cc.  Sol.  cc.  Solution. 

o  o.oo  0.0017 

0.58  3-48  0-0048 

2.89  17-34  0-0058 

5-79  34-74  0.0064 

The  residues  were  dried  at  70°  C. 
CALCIUM    OXIDE.     See  Calcium  Hydroxide,  p.  91. 
CALCIUM    PHOSPHATE    (Tribasic)    Ca3(PO4)2. 
SOLUBILITY  IN  WATER. 

The  determinations  of  the  solubility  of  this  salt  in  water,  as  stated 
in  the  literature,  are  found  to  vary  within  rather  wide  limits,  due,  no 
doubt,  to  the  fact  that  so-called  tribasic  calcium  phosphate  is  apparently 
a  solid  solution  of  the  dibasic  salt  and  calcium  oxide,  and  therefore 
analyses  of  individual  samples  may  show  an  excess  of  either  lime  or 
phosphoric  acid.  When  placed  in  contact  with  water,  more  PO4  ions 
enter  solution  than  Ca  ions,  the  resulting  solution  being  acid  in  reaction 
and  the  solid  phase  richer  in  lime  than  it  was,  previous  to  being  added 
to  the  water.  For  material  having  a  composition  approximating 
closely  that  represented  by  the  formula  Ca3(PO4)2  the  amount  which 
is  dissolved  by  CO2  free  water  at  the  ordinary  temperature,  as  cal- 
culated from  the  calcium  determination,  is  o.oi  to  o.io  gram  per  liter, 
depending  upon  the  conditions  of  the  experiment.  Water  saturated 
with  CO2  dissolves  0.15  to  0.30  gram  per  liter. 

A  list  of  references  to  papers  on  this  subject  is  given  by  Cameron 
and  Hurst  —  J.  Am.  Chem.  Soc.  26,  903,  '04;  see  also  Cameron  and 
Bell,  Ibid.  27,  1512,  '05. 


CALCIUM    PHOSPHATE 
CALCIUM 


96 


PHOSPHATE    (Dibasic)    CaHPO4.2HaO. 
SOLUBILITY  IN  WATER. 

(Cameron  and  Seidell  —  J.  Am.  Chem.  Soc.  26,  1460,  '04;  see  also  Rindell  —  Compt.  rend.  134,  112,  'oa; 
Magnanini  —  Gazz.  chim.  ital.  31,  II,  544,  '01.) 

i  liter  of  CO2  free  water  dissolves  0.136  gram  CaHPO4  at  25°. 

i  liter  of  water  sat.  with  CO2  dissolves  0.561  gram  CaHPO4  at  25°. 

SOLUBILITY  OF  Di  CALCIUM  PHOSPHATE  AND  OF  MONO  CALCIUM  PHOS- 
PHATE IN  AQUEOUS  SOLUTIONS  OF  PHOSPHORIC  ACID  AT  25°. 

(Cameron  and  Seidell  —  J.  Am.  Chem.  Soc.  27,  1508,  '05;  Causse  —  Compt.  rend.  114,  414,  '92.) 

2O5 

in  Excess  of 

that  combined 

with  Ca. 

2.53     CaHP04.2H20 
21.5 

46.45 

89.0 
128.0 
159-4 


Gram,  .per  Liter  of  ^         ^  ^.per  Liter 


Solution. 

CaO. 

P2O5. 

I.7I 

4.69 

n-57 

36.14 

23-3I 

75-95 

39.81 

139.6 

49.76 

191  .0 

59-40 

234.6 

70.31 

279.7 

77.00 

317.0 

72.30 

35J-9 

69-33 

361.1 

59.98 

419.7 

53-59 

451  .7 

44-52 

505-8 

39-89 

538.3 

Calc.  from 


Found. 

CaHPO. 


c  r.  T>, 
Sohd  Phase' 


190.7 

tt 

226.0 

122.2 
169.0 

CaHP04.2H20+ 
CaH4(PO  )2.H20 
CaH4(P04)2.H20 

I86.I 

tt 

267.9 

a 

3I6.I 

" 

393-1 

tt 

437-4 

" 

4-i5 
28.05 

56-53 
97.01 
120.7 
144.1 
170.6 

(174.2       CaHPO4  or 
I32i.3       CaH4(P04)2 
301.6       CaH4(P04)2 
289.3 
250.2 
223.7 
185.8 
166.4 
Density  of  the  solution  in  contact  with  both  salts  at  25°  =  1.29. 

SOLUBILITY  OF  Di  CALCIUM  PHOSPHATE  IN  AQUEOUS  N/2oo  SOLUTION 
OF  ACID  POTASSIUM  TARTRATE  AT  25°. 

(Magnanini .) 

i  liter  of  the  solution  contains  0.08  gram  Ca  =  0.235  gram  CaHPO4. 

CALCIUM    PHOSPHATE    (Monobasic)    CaH4(PO4)2,H2O. 

SOLUBILITY  IN  WATER. 

This  salt  is  stable  in  contact  with  the  aqueous  solution  only  when 
there  is  present  free  phosphoric  acid  to  the  extent  indicated  by  the 
above  table. 

CALCIUM    PELARGONATE    (Nonate)  Ca[CH3(CH2)7COO]2.H2O. 
CALCIUM    PROPIONATE    Ca(CH3.CH2COO)2.H2O. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Lumsden  —  J.  Chem.  Soc.  81,  355,  '02;  Krasnicki  —  Monatsh.  Chem.  8,  597,  '87.) 


Calcium  Pelargonate. 

Grams 

t°.  Ca[CH3(CH2)7COO]2 

per  100  Grams  H2O. 

o  0.16 

20  0.14 

40  0.13 

60  O.I2 

80  0.15 

90  0.18 

ioo  0.26 


Calcium  Propionate. 

Grams  Ca(CH3.CH2COO)2  per  100  Grams. 

Water.  Solution. 

42.80  29.97 

39.85  28.48 

38.45  27.76 

38.25  27.67 

39.85  28.48 

42.15  29.66 

48.44  32-63 


97  CALCIUM    SELENATE 

CALCIUM     SELENATE    CaSeO4. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  532,  '94.) 
t°.  -i°.  +5°.  20°.  37°.  67°. 

Cms.  per  ioo  gms.  sol.  7.4        7.3        7.6        6.8        5.1 

The  accuracy  of  these  results  appears  questionable. 

CALCIUM    SILICATE    CaSiO3. 
SOLUBILITY  IN  WATER  AND  IN  AQUEOUS    SUGAR  SOLUTIONS  AT  17°. 

(Weisberg  —  Bull.  soc.  chim.  [3]  15,  1097,  '96.) 

The  sample  of  calcium  silicate  was  air  dried. 

Grams  per  ioo  cc.  Saturated  Solution. 


Solvent. 

Water 
10%  sugar  sol. 
20%  sugar  sol. 

A 

LI7°- 

After  Boiling  and  Filtering  Hot. 
CaO(det.)        CaSiO.,(calc.) 

0.0094           0.0195 
O-OI2O            O.O249 

CaO(det.) 

o  .  0046 

0.0065 
0.0076 

CaSiO3(calc.) 
0.0095 
0-0135 
0.0157 

CALCIUM    SUCCINATE    Ca(C2H2O2)2. 
CALCIUM    (Iso)    SUCCINATE    CaCH3.CHC2O4.H2O. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Miczynski  —  Monatsh.  Chem.  7,  261,  '86.) 

Calcium  Succinate.  Calcium  Iso  Succinate. 


te. 

Gms. 
Ca(C2H202)2 
per  ioo  Gms. 

Gms. 
to     Ca(C2H202)2 
'    per  ioo  Gms. 

Gms. 
to    Ca(C2H202)2 
'  per  ioo  Gms. 

Gms. 
to     Ca(C2H2O2)2 
'    per  ioo  Gms. 

H2O. 

H2O. 

H20 

H20. 

0 

I  .127 

50 

1.029 

O 

0.522 

50 

0.440 

10 

1.220 

60 

0.894 

IO 

0.524 

60 

0.396 

20 

1.276 

70 

0-770 

20 

o-s1; 

70 

0.342 

40 

I.I77 

80 

0.657 

40 

o-475 

80 

0.279 

ioo  cc.  H2O  dissolve  1.424  grams  succinate  (CaC4H4O4.H2O)  at  18°, 
and  1.436  grams  at  25°. 

ioo  cc.  95%  alcohol  dissolve  0.00136  gram  succinate  (CaC4H4O4. 
H2O)  at  18°,  and  0.00136  gram  at  25°. 

(Partheil  and  Hiibner  —  Archiv.  Pharm.  241,  413,  '03.) 

CALCIUM    SULPHATE    CaSO4.2H2O. 

SOLUBILITY  IN  WATER. 

(Hulett  and  Allen  —  J.  Am.  Chem.  Soc.  24,  674,  '02;  for  references  to  other  determinations  see  Hulett 
and  Allen,  also  Euler — Z.  physik.  Chem.  49,  313,  '04.  Determinations  by  the  electrolytic  conductivity 
method  Holleman,  Kohlrausch  and  Rose  —  Z.  physik.  Chem.  12,  129,  241,  '93.) 


Gms.  CaSO4 

Millimols. 

Density  of             >0 

Gms.  CaSO4 

Millimols 

Density  of 

t   . 

per  ioo  cc. 
Solution. 

per 

Liter. 

Solutions. 

per  ioo  cc. 
Solution. 

per  Liter. 

Solutions. 

0 

0-1759 

12 

.926 

I 

.00197 

40 

O 

.2097 

I5-4I3 

C 

•99439 

10 

0-1928 

14 

.177 

I 

•00173 

55 

O 

.2009 

I4-765 

0 

.98796 

18 

0.2016 

14 

.817 

I 

.00059 

65 

3  ° 

.1932 

I4.2OO 

0 

.98256 

25 

o  .  2080 

15 

295 

0 

.99911 

75 

0 

.1847 

J3-575 

0 

.97772 

30 

o  .  2090 

15 

.361 

0 

.99789 

IOO 

o 

.1619 

ii  .900 

35 

o  .  2096 

15 

405 

O 

.99789 

107 

n-390 

... 

CALCIUM    SULPHATE  98 

SOLUBILITY  OP  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC, NITRIC,  CHLOR  ACETIC,  AND  FORMIC  ACIDS. 

(Banthisch  —  J.  pr.  Chem.  29,  52,  '84;  Lunge  —  J.  Soc.  Chem.  Ind.  4,  32,  '85.) 

In  Hydrochloric.  In  Nitric.    In  Chlor  Acetic.  In  Formic. 


Grams  Acid 
per  100  cc. 

Grams  CaSO4  per 
100  cc.  Sol. 

Gms.  CaSO4  per 
100  cc.  Solution 

Gms.  CaSO4  per 

100  CC.  Sol. 

Gms.  CaSO4  per 
loo  cc.  Sol. 

Solution. 

at  25°. 

at  io26. 

at  25°. 

at  25°. 

at  25°. 

O 

0.208 

0.160 

O.2O8 

O.2O8 

0.208 

I 

0-72 

1.38 

0.56 

2 

I  .02 

2.38 

0.82 

3 

1.25 

3.20 

I  .02 

4 

1.42 

3-64 

I  .20 

O.22 

0.24 

6 

1.65 

4-65 

1.48 

8 

i-74 

1.70 

10 

.  .  . 

1.84 

0.25 

12 

I.98 

SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  PHOS- 
PHORIC ACID  AT  25°. 

(Taber  —  page  61,  Bull.  33,  Bureau  of  Soils  —  U.  S.  Dept.  Agr.,  1906.) 


Gms. 

per 

Liter. 

Sp.  Gr.  of 

Gms.  per  Liter.                    gp   QT  of 

P204. 

CaSO4. 

Solutions  at  §f  . 

P205. 

CaSO4-             Solutions  at  ff  . 

0 

.0 

2 

126 

O 

.9991 

145 

.1 

7 

.920 

.106 

5 

•  O 

3 

143 

I 

•  OO2 

205 

.0 

8 

•383 

•145 

10 

•5 

3 

734 

I 

.007 

311 

•5 

7 

•965 

.221 

21 

•4 

4 

456 

I 

•  Ol6 

395 

.8 

6 

.848 

.280 

46 

•3 

r 

760 

I 

•035 

494 

.6 

5 

•572 

•344 

05 

•3 

H 

318 

I 

•075 

SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  SUL- 
PHURIC ACID. 

(Cameron  and  Breazeale  —  J.  Physic.  Chem.  7,  574,  '03.) 


Grams  H2SO4 

Resul 

Its  at  25°. 

Results  at  35°, 

,      Results  at  43°  , 

per  Liter  of 
Solution. 

Gms.  CaSO4 
per  Liter. 

wt.  of  i  cc: 

Sol. 

Gms.  CaSO4 
per  Liter. 

Gms.  CaSO4 
per  Liter. 

O-OO 

2  .126 

0.9991  grams 

.  .  . 

2.145 

0.48 

2.128 

1.0025     " 

2.209 

2.236 

4-87 

2.144 

1.0026     " 

2.451 

2.456 

8.  ii 

2.203 

1.0051     " 

2.760 

16.22 

2.382 

1.0098     " 

3.II6 

48.67 

2.727 

i  .0302     " 

3-397 

3-843 

75.00 

2.841 

I-Q435     " 

.  .  . 

4.146 

97-35 

2-779 

1.0756     " 

3.606 

146.01 

2-571 

u 

3-J5o 

4-139 

194.70 

2-3*3 

1.1134     " 

3-551 

243-35 

i  .901 

1.1418     " 

2-959 

292.02 

i-54i 

1.1681     " 

,  .  . 

2.481 

99 


CALCIUM    SULPHATE 


SOLUBILITY  OF  CALCIUM   SULPHATE   IN  AQUEOUS   SOLUTIONS   OF 
AMMONIUM   SALTS. 

(In  NH4C1  and  NH4NO3,  Cameron  and  Brown  —  J.  Physic.  Chem.  9,  210,  '05  ;  In  (NH4)2SO4  at  25*, 
Sullivan  —  J.  Am.  Chem.  Soc.  27,  529,  '05;  In  (NH4)2SO4  at  50°,  Bell  and  Tabor  —  J.  Physic.  Chem.  10, 
119,  '06.) 


In  NH4C1      In  NH4NO3                   In  NH4C1 
at  25°.             at  25°.                           at  25°. 

Gms.  Ammo-              G.CaSO4                G.  CaSO4         Gms.  Ammo-     G.  CaSO4 
nium  Salt                  Dissolved                 Dissolved              nium  Salt        Dissolved 
per  Liter.                  per  Liter.                 per  Liter-              per  Liter.       per  Liter. 

o                   2.08                 2.08               300         10.10 
20                  5.00                3.70              375           7.40 
40                 7  .00               5  .10             400 
60                  8  .  oo                6  .  05              600 
80                  8.50                7.00              800 
100                  9.10                7  .65             1000 
150                10.30                8.88            1400 
200                10-85                9-85            sat. 

In  (NH4)2SO4  at  25°.                              In  (NH4)^SO4 

Grams  per  Liter  Sol.          \vt.  of  100  cc.                        Grams  per  Liter  Sol. 

In  NH4N 

at  25°. 

G.  CaSO4 
Dissolved 
per  Liter. 

I0.8o 

II  -40 
12.15 
12  .IO 
II.  8l 
IO.02 

7-55 
at  50°. 

Sp.  Gr. 

(NH4)2SO4. 

CaSO4. 

Sat, 

Sol. 

'(NH4)2S04. 

CaSO4. 

of  Solutions. 

O-OO 

0 

.208 

99 

.91 

O 

.OO 

2 

.168 

0.129 

0 

.204 

99 

.91 

15 

•65 

I 

.609 

I  .0026 

0.258 

0 

.199 

99 

.92 

30 

•67 

I 

•750 

I.OII3 

0.821 

0 

.181 

99 

•95 

91 

.6 

2 

•542 

I  .0440 

1.643 

0 

.166 

99 

•99 

160 

•4 

3 

.402 

I  -0819 

3.287 

0 

•  154 

IOO 

.10 

221 

.6 

4 

.068 

1.1108 

6-575 

0 

.144 

IOO 

•34 

340 

.6 

5 

.084 

i  .1653 

13  .15 

0 

.146 

IOO 

.82 

4l6 

•5 

5 

•354 

i  .  1964 

26.30 

o 

.162 

101 

.76 

428 

•4 

4 

.632 

i  .  2043 

84-9 

0 

233 

105 

•34 

530 

.8 

2 

.152 

1-2437 

169.8 

0 

333 

no 

•32 

566 

,o 

I 

.08 

1.2508 

339-6 

0 

45° 

119 

,15                     566.7 

0 

.00 

i  .2510 

SOLUBILITY  OF  CALCIUM   SULPHATE  IN  AQUEOUS   SOLUTIONS   OF 
CALCIUM   SALTS  AT  25°. 


(Cameron  and  Seidell  —  J.  Physic.  Chem.  5,  643,  '01;  Seldell  and  Smith  —  Ibid.  8,  493,  '04;  Cameron 
and  Bell  —  J.  Am.  Chem.  Soc.  28,  1220,  '06.) 

In  Calcium                  In  Calcium               In  Calcium  Hydroxide  and 
Chloride.                         Nitrate.                                   vice  versa. 

Grams  per  Liter  Sol. 

Gms.  per  Liter  Sol. 

Wt.  of 

Gms.  per  Liter  Sol. 

Solid 

CaCl2. 

CaSO4.  ' 

Ca(N03)2. 

CaS04. 

i 

cc.  Sol. 

CaO. 

CaSO4. 

Phase. 

0-00 

2 

.06 

0-0 

2.08 

0 

.998 

O 

•  O 

2 

.126 

CaSO^HjO 

7-49 

I 

.24 

25 

1.24 

I 

.014 

O 

.062 

2 

•030 

u 

II  .96 

I 

.18 

50 

I  .20 

I 

.032 

0 

.I76 

I 

.918 

tt 

25-77 

I 

.  IO 

IOO 

I-I3 

I 

.067 

0 

•349 

I 

•853 

« 

32-05 

I 

.08 

2OO 

o-93 

I 

•137 

O 

.61 

j 

.722 

it 

SI-S3 

I 

.02 

300 

0.7-6 

I 

.204 

0 

•939 

I  . 

634 

a 

97.02 

0 

.84 

4OO 

o-57 

I 

.265 

I 

.222 

j 

.588 

\  CaS04.2H20+ 
!      Ca(OH)2 

192.71 

0 

•47 

500 

0.40 

I 

.328 

I 

.242 

I 

.214 

Ca(OH)2 

280.30 

0 

.20 

544 

o-35 

I 

•352 

I 

•150 

0 

.666 

a 

367-85 

0 

•03 

I 

.166 

0 

.00 

it 

CALCIUM  SULPHATE 


100 


SOLUBILITY    OF    CALCIUM    SULPHATE    IN   AQUEOUS    SOLUTIONS    op 
MAGNESIUM   CHLORIDE  AND  OF  MAGNESIUM  NITRATE  AT  25°. 

(Cameron,  Seidell,  and  Smith.) 

In  Magnesium  Chloride.  In  Magnesium  Nitrate. 

Grams  per  Liter  of  Sat.  Solution. 


MgCl2. 

CaSO4. 

H2Oo 

O-O 

2.08 

997-9 

8.50 

4.26 

996-5 

19.18 

5-69 

994-5 

46.64 

7-59 

989.1 

121  .38 

8.62 

972.2 

206.98 

6-57 

949-9 

337-o 

2.77 

908.7 

441.1 

i-39 

878.6 

Gms.  per 

Liter  Sol. 

Wt.  of  i  cc. 
Solution. 

0.9981 

Mg(N03)2- 

o.o 

CaSO4. 
2.08 

25 
50 
100 
200 

5-77 
7.88 
9.92 
13-34 

I  .0205 
1.0398 
1.0786 
I  .1498 

300 
40O 

14.00 
14.68 

I.2I90 
I  .2821 

5*4 

15.04 

!-3553 

SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  MAG- 
NESIUM SULPHATE  AT  25°. 

(Cameron  and  Bell  —  J.  Physic.  Chem.  10,  210,  '06.) 


Grams  per  Liter  Solution.              5 

>p.  Gr.  of 
itions  at  if 

MgS04. 

CaS04. 

o.o 

2.046                 1.0032 

3-20 

1.620                 I-0055 

6-39 

I-507 

.0090 

10.64 

I.47I 

-OIl8 

21.36 

1.478 

.0226 

42.68 

I-558 

.0419 

64.14 

I.  608 

.0626 

85.67 

I  .617 

•0833 

128.28 

1.627                 ] 

.II9O 

Grams  per  Liter  Solution. 


MgS04. 
149.67 
I65-7 

CaS04. 

•597 
•549 

171  .2 
198.8 

•474 
.422 

232.1                ] 
265.6                ] 
298.0               < 

•254 
•  070 
>.86o 

330.6               < 

5.647 

355-o          < 

5.501 

Sp.  Gr.  of 
Solutions  at  j|f0. 

•J377 
.1479 

•1537 
.1813 

.2095 
.2382 
.2624 
.2877 
•3023 


SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  POTAS- 
SIUM CHLORIDE,  BROMIDE,  AND  IODIDE  AT  21°. 

(Ditte  —  Ann.  chim.  phys.  [7]  14,  294,  '08.) 

In  KC1  Solutions.  In  KBr  Solutions.  In  KI  Solutions. 


Grams  of  the 
Potassium  Salt 
per  Liter. 

Cms.  CaSO4 
per  Liter. 

O 
10 

2.05 

3-6 

2O 
40 
60 

4-5 
5-8 
6.6 

80 

7-2 

100 

I25 

7-5 
double  salt 

200 

250 

300 


Cms.  CaSO4 
per  Liter. 

2.O5 

3-i 
3-6 
4-5 
5-2 
5-9 
6-3 
6.7 

7-o 

7-3 
double  salt 


Gms.  CaSO4 
per  Liter. 

2.05 
2.8 

3-2 
3-9 
4-5 
4-85 

5-45 
5-8 

5-95 

6-00 

double  salt 


ioi  CALCIUM    SULPHATE 

SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  POTAS- 
SIUM NITRATE  AND  OF  POTASSIUM  SULPHATE  AT  25°. 

(Seidell  and  Smith  —  J.  Physic.  Chem.  8,  493,  '04;  Cameron  and  Breazeale  —  Ibid.S,  335,  '04.) 

In  Potassium  Nitrate.  In  Potassium  Sulphate. 

Cms.  per  Liter  Cms.  per  Liter 

Solution.                 Wt.oficc.                                   Solution.  Wt.  of  i  cc. 

Solution.  ^r—— '  .  Solution. 


KNO3-       CaSO4.  K2SO4.        CaSO4. 

o.o       2.08         0.9981  o.o         2.08        0.9981 

12-5    3-28     I.OoSl  4.88    I. 60     1.0036 

25.0    4.08     I.OI54  5.09    1.56     1.0038 

50.0    5.26     I.032I  9.85    1.45     1.0075 

loo-o   6.86  1.0625  I9-57  *-49  1.0151 

150    7.91  1.0924  28.35  1.55  1.0229 

200    8.69  1.1224  30.66  1.57  1.0236 

260   syngenite  1-1539  32-47  1-58* 

*  Solid  phase  syngenite.     Results  for  the  solubility  of  syngenite  in  solutions  of  potassium  sulphate  are 
also  given  in  the  original  paper. 

SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  CHLORIDE  AT  26°. 

(Cameron  —  J.  Physic.  Chem.  5,  556,  '01;  see  this  paper  for  references  toother  work,  also  Orloff — T.russ- 
phys.  chem.  Ges.  37,  949,  '02;  Cloez  —  Bull.  soc.  chim.  [3]  29,  167,  '03;  d'Anselme  —  Ibid.  [3]  2Q» 
372,  '03.) 

Grams  per  100  cc.  Solution.       \vt.  of  i  cc.  Grams  per  100  cc.  Solution.     \yt  of  i  cc. 

'NaCl.  CaS04.    '         Solution.  '     NaCl.  CaSO4.  '          Solution.' 

0-00  0.2I2I  0.9998  I7-650         0.712  1.1196 

9.115   0.666    1.0644       22.876   0.679    1.1488 
14.399   0.718    1.0981       26.417   0.650    1.1707 

14.834    0.716      I.IOI2          32.049    0.572     I-2034 

SOLUBILITY  OF  MIXTURES  OF  CALCIUM  SULPHATE  AND  CALCIUM  CAR- 
BONATE IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE  AT  23°. 

(Cameron  and  Seidell  —  J.  Physic.  Chem.  5,  643,  '01.) 

Grams  per  Liter  Solution.  Grams  per  Liter  Solution. 

NaCl.          CXHC03)2.         CaSC4.  "~  NaCl.          Ca(HCO3)2.         CaSO47 

o.oo  0.060  J-93o  79  -52  0.060  6.424 

3.63  0.072  2.720  121.90  0.056  5-272 

11.49  0-089  3-446  193.80  0.048  4.786 

39.62  o-ioi  S^S^  267.60  0.040  4.462 

SOLUBILITY  OF  MIXTURES  OF  CALCIUM  SULPHATE  AND  SILVER  SUL- 
PHATE IN  WATER. 

(Euler  —  Z.  physik.  Chem.  49,  313,  '04.) 


... 

Per  Liter 

of  Solution. 

Total  Salt           «     r_     . 
1JS2"-        %&* 

'  Gms.  Salt. 

Gms.  Equiv. 
Salt. 

17o|CaSO< 

2.  SI 

7-235 

0-034 
0-0464 

0-9473         1-0083 

0<CaSO, 
25   Ug2S04 

2.61 
8.  ii 

0.0383 
0.0520 

1.062           i.  oio 

CALCIUM  SULPHATE  102 

SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  NITRATE  AND  OF  SODIUM  SULPHATE  AT  25°. 

(Seidell,  Smith,  Cameron,  Breazeale.) 

In  Sodium  Nitrate.  In  Sodium  Sulphate. 

Grams  per  Liter  Solution.  \vt.  of  i  cc.  Grams  per  Liter  Solution.  \yt.  of  i  cc. 

NaN03.     CaS04.  Solution.  '  Na2SO4."   CaSO4.  Solution. 

o     2.08  0.9981  2.39     1.65  1.0013 

25       4.25  1.0163  9.54       1.45  1.0076 

50  5.50  1-0340  14-13  r-39  1-0115 

100  7.10  1.0684  24-37  J-47  1-0205 

200  8.79  1.1336  46-15  1-65  1-0391 

300  9.28  1.1916  115.08  2.10  1-0965 

600  7.89  I-3^>39  146.61  2.23  1.1427 

655  7.24  i-39°4  257.10  2.65  i. 2120 

SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  AND  ALCOHOLIC 
MONO  POTASSIUM  TARTRATE  SOLUTIONS  AT  20°. 

(Magnanini  —  Gazz.  chim.  ital.  31,  II,  544,  '01.) 

Gms.  CaSO4  Cms.  CaSO.4 

Solvent.  per  100  Gms.  Solvent.  per  100  Gms. 

Solution.  Solution 

Water  0.2238     10%  alcoholic  N/2oo  KHC2H4O6       0.0866 

Aq.  N/200  KHC4H4O6  0.2323     Aq.  N/2oo  KHC2H4O6  +  5% 

10  per  cent  alcohol  0.0970         tartaric  ac.  0.2566 

10%  ale.  NAoo  KHC2H406  +  5% 

tartaric  ac.  o .  1086 

SOLUBILITY  OF  CALCIUM  SULPHATE  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Stolle  — Z.  Ver.  Zuckerind.  50,  331,  'oo.) 

Per  cent  Concen-  Grams  CaSO4  Dissolved  by  i  Liter  of  the  Sugar  Solutions  at: 

tration  of  Sugar 
Solutions. 

O 
IO 
20 
27 

35 
42 

49 

55 

CALCIUM    SULPHIDE    CaS. 

SOLUBILITY  IN  AQUEOUS  SUGAR  SOLUTIONS. 


2 

I 

I 
I 

30°. 

.041 
.808 

.263 
.030 

2 
I 

I 
I 
I 

0 
0 

40°. 

•T57 
•730 
.652 

•438 
•050 

•564 
.486 

i 
i 
i 

i 

0 
0 
0 

50°. 

•730 
•730 
.419 

.088 

•777 
•739 
•505 

i 
i 
i 

i 
i 

0 
0 
0 

60°. 

•730 

•574 
.380 
.283 
.108 
.816 

•564 
.486 

i 
i 
i 
i 

0 
0 
0 

o 

70°. 
.652 

•574 
.419 
•283 
.914 

•855 
.603 

•369 

i 

i 
i 

0 

0 
0 
0 

80°. 

.710 

.613 

•263 
.972 

•729 

.486 

.330 

Per  cent  Concen- 
tration  of  Sugar     /• 

(Stolle.) 
Grams  CaS  Dissolved  per  Liter  of  the  Sugar  Solutions  at: 

Solutions. 

30°. 

40°. 

50°. 

60°. 

70°. 

80°. 

90°: 

O 

i 

.982 

2 

.123 

I 

•235 

1.390 

I  .696 

2 

.032 

2.496 

10 

i 

.866 

I 

.3l6 

I 

.441 

1.673 

I  .560 

I 

•634 

1-544 

20 

2 

.187 

I 

.696 

I 

.802 

1.905 

1.879 

I 

.892 

1.930 

27 

2 

.522 

2 

.097 

2 

•059 

2  .226 

2.342 

2 

•304 

2-357 

35 

2 

.689 

2 

.265 

2 

.304 

2.406 

2-342 

2 

•857 

2-947 

42 

2 

•342 

2 

-I36 

2 

.226 

2.522 

2-574 

2 

•509 

2.689 

49 

2 

•445 

2 

.290 

2 

•458 

2.638 

2.728 

2 

.8l8 

3-063 

55 

2 

•509 

2 

.226 

2 

•340 

2.882 

2.766 

2 

•972 

3.616 

103  CALCIUM    SULPHITE 

CALCIUM     SULPHITE    CaSO3. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SUGAR  SOLUTIONS  AT  18°. 

(Weisberg  —  Bull.  soc.  chim.  [3]  15,  1097,  '96.) 

Grams  CaSOa  per  100  cc.  Solution. 
Solvent.  '   A      Ro  After  Boiling 

Solution  2  Hours. 

Water  o .  0043 

10  Per  cent  Sugar  0-0083  0.0066 

30  Per  cent  Sugar  0.0080  0-0069 

CALCIUM    TARTRATE     CaC4H4O6.4H2O. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder  —  Bull.  soc.  chim.  [3]  33,  747,  '05.) 

-o      Cms.  CaC4H4O6.4H2O   ±0    Gms.CaC4H4O6.4H2O          .0    Gms.CaC4H4O6.4H2O 
per  100  cc.  Sol.  per  100  cc.  Sol.  per  100  cc.  Sol. 

o  0-0365  30  0-0631  70  0.1430 
10  0-0401  40  0-0875  80  0-1798 
20  0-0475  5°  o-iioo  85  0.2190 

25  0-0525  60  O.I262 

ioo  gms.  aq.  Ca.  tartrate  solution  contain  0.0185  g.  CaC4H4O6.4H2O 
at  18°,  and  0.029489  at  25°. 

ioo  gms.  95%  alcohol  solution  contain  0.0187  g.  CaC4H4O6.4H2O  at 

l8°,   and  0.02352   at   25°.  (Partheil  and  Hiibner  —  Archiv.  Pharm.  241,  413,  '03.) 

ioo  gms.  aq.  Ca.  tartrate  solution  contain  0.0364  g.  CaC4H4O6  at  20°. 
ioo  gms.  10%  alcohol  solution  contain  0.0160  g.  CaC4H4Oc  at  20°. 
ioo  gms.  10%  alcohol  +  5%  tartaric  acid  solution  contain  0.1632  g. 

CaC4H4O6  at  200.  (Magnanini  —  Gazz.  chim.  ital.  31,  II,  544,  ?oi.) 

SOLUBILITY  OF  CALCIUM  TARTRATE  IN  AQUEOUS  ACETIC  ACID 
SOLUTIONS  AT  26°-27°. 

(Herz  and  Muhs  —  Ber.  36,  3715,  '03;  see  also  Enell  —  Pharm.  Centrallh.  38,  181;  Z.anal.  Chem.  38, 

368,  '99-) 

Normality  of    Gms.CH3COOH     Residue  from  Normality  of    Gms.CH3COOH     Residue  from 

Acetic  Acid.       per  ioo  cc.  Sol.     50.052  cc.  Sol.  Acetic  Acid,    per  ioo  cc.  Sol.     50.052  cc.  Sol. 

o  o  0-0217  3 .80  22.80  0.2042 

0.57  3.42  0-1082  5.70  34-20  0-1844 

1.425  8.55          0-1635  10.09  60.54  0-1160 

2.85  17.10          0.1970  16.505  93 .03  0.0337 

The  residue  was  dried  at  70°  C. 

CALCIUM    BITARTRATE     CaH2(C4H4O6)2. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS    SOLUTIONS  OF  ACIDS  AND 

OF  SALTS. 

(Warington  —  J.  Chem.  Soc.  28,  946,  '75.) 

In  Hydrochloric  Acid.       In  other  Acids  and  in  Salt  Solutions  at  14°. 

<^*a  g^J!:glS&         AcidorSau.    ^^S.0 

ioo  Gms.  Sol.       At  22°.         At  80°. 

o  0.600  4.027  Acetic  Acid  0-81  0.422 

0.68  3.01  5.35  Tartaric  Acid  1.03  0.322 

2.15  6.88  n-35  Citric  Acid  0.84  0.546 

4.26  11.19  20.23  Sulphuric  Acid  0-685  1.701 

8.36  22.75  40-93  Hydrochloric  Acid  0.504  1-947 

16.13  48.31  80.12  Nitric  Acid  0.845  1.969 

Potassium  Acetate  1-387  0.744 

ITObhartrlt?aff0olveo'422gms'  Potassium  Citrate  1.397  0.843 


CALCIUM    VALERATE  104 

CALCIUM    VALERATE    Ca[CH3(CH2)3COO]2.H2O. 
CALCIUM  (Iso)  VALERATE    Ca[(CH3)2.CH.CH2.COO]2.3H2O. 
SOLUBILITY  OP  EACH  IN  WATER. 

(Lumsden  —  J.  Chem.  Soc.  81,  355,  '02;  see  also  Furth  —  Monatsh.  Chem.  9,  313,  '88;  Sedlitzky  — 

Ibid,  8,  566,  '87.) 

Calcium  Valerate.  Calcium  Iso  Valerate. 

Solid 
Phase. 

Ca(C5H902)2.5H20 


Gms.  Ca(( 

:5HBO2)2                            Gms.  Ca(C5H9O2)2 

t°,             per  TOO  Gms.                 t  °. 

per  100  Gms. 

Water.     Solution. 

Water. 

Solution. 

O 

9.82 

8.94 

o 

26.05 

2O-66 

10 

9-25 

8-47 

10 

22.70 

18.50 

20 

8.80 

8.09 

20 

21.  80 

17.90 

30 

8-40 

7-75 

30 

21.68 

17.82 

40 

8.05 

7-45 

40 

22  .OO 

18.18 

50 

7-85 

7.28 

45-5 

22-35 

18.42 

57 

7-75 

7.19 

J9-95 

16.63 

60 

7.78 

7.22 

60 

18.38 

I5-52 

70 

7-80 

7.24 

70 

17.40 

14.82 

80 

7-95 

7-36 

80 

16.88 

14.44 

90 

8.20 

7-58 

90 

16.65 

14.28 

100 

8.78 

8.07 

100 

l6-55 

14  .  20 

CAOUTCHOUC. 

Ca(C5H902)2.H20 


SOLUBILITY  IN  ORGANIC  SOLVENTS. 

(Hanausek  —  J.  pharm.  chim.  [5]  15,  509,  '87.) 

Grams.  Caoutchouc  Dissolved  per  100  Gms.  Solvent. 

Solvent.  , ; ^ , 

Gear  a.          Tete  Noire.      Sierra  Leone. 

Ether  2.5  3.6  4.5 

Turpentine  4.5  5.0  4.6 

Chloroform  3.0  3.7  3.0 

Petroleum  1.5  4.5  4.0 

Benzene  4.4  5.0  4.7 

Carbon  Bisulphide  0.4  o.o  o.o 

CAMPHORIC    ACID    C8H14(COOH)2. 

100  grams  of  water  dissolve  0.8  gram  C8H14(COOH)2  at  25°,  and  10 
grams  at  the  b.  pt.  (U.S. P.) 

CARBAZOLE  (Di  Phenylene  imid)  (C6H4)2NH. 

100  grams  abs.  alcohol  dissolve  0.92  gms.  (C6H4)2NH  at  14°,  and 
3.88  grams  at  b.  pt. 

100  grams  toluene  dissolve  0.55  gm.  (C6H4)2NH  at  16.5°,  and  5.46 
grams  at  b.  pt. 

CARBAMIDES. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

as  Methyl  Phenyl  Carbamide  (m.  pt.  82°),  Benzyl  Carbamide  (m.  pt. 
149°)-  o  Tolyl  Carbamide(m.pt.  185°)  and  p Tolyl  Carbamide (m.pt.  173°). 

(Walker  and  Wood  —  J.  Chem.  Soc.  73,  626,  '98.) 

Grams  Carbamide  per  100  cc.  Sat.  Solution. 


v 

as 

Methyl 

Phenyl. 

Benzyl. 

P  Tolyl. 

0 

Tolyl. 

Water 

45 

74 

I.7I 

0.307 

0 

.251 

Acetone 

23 

29. 

4 

3-10 

2.66 

O 

.462 

Ether 

22 

•5 

2  . 

28 

0-053 

O.O62 

O 

.Ol62 

Benzene 

44 

2 

12  . 

4 

0.0597 

0.043 

o 

•0155 

CARBON    DIOXIDE 


CARBON    DIOXIDE    CO2. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SODIUM  CHLORIDE  SOLUTIONS. 

(Bohr  — Wied.  Ann.  Physik.  [3]  68,  503,  '99;  Geffcken  —  Z.physik.Chem.  49,  271,  '04;  Just  —  Ibid. 

37,  354i  '°i.) 
Solubility  in  Water. 


b  . 

0. 

ft. 

/. 

o 

o-335 

i-7J3 

5 

0.277 

1.424 

10 

0.231 

1.194 

15 

0.197 

1.019 

1.070 

20 

0.169 

0.878 

25 

0.145 

0-759 

0.826 

30 

0.126 

0.665 

40 

0.097 

0-530 

50 

0.076 

0.436 

60 

0.058 

0-359 

Nac1% 

In  17.62% 
Nad. 

1.234 

0.675 

I  .024 
0-875 

o-577 
0-503 

o-755 
0.664 

0-583 

0.442 
o-393 

0-5*7 
0.414 

0.319 
0.263 

0.370 
0-305 

0-235 
0.183 

q  =  wt.  of  gas  dissolved  by  100  grams  of  solvent  at  a  total  pressure  of  760  mm. 

0  =  the  Bunsen  Absorption  Coefficient  which  signifies  the  volume  (v)  of 
the  gas  (reduced  to  o°  and  760  mm.)  taken  up  by  unit  volume  (F)  of  the  liquid 
when  the  pressure  of  the  gas  itself  minus  the  vapor  tension  of  the  solvent  is 
760  mm.  _  v 

~  V(i  +  0.00367  /)  ' 

/  =  the  Ostwald  Solubility  Expression  which  represents  the  ratio  of  the 
volume  (v)  of  gas  absorbed  at  any  pressure  and  temperature,  to  the  volume 


(V)  of  the   absorbing  liquid,  i.e.  I  =  —• 


This  expression  differs  from  the 


Bunsen  Absorption  Coefficient,  /3,  in  that  the  volume  (v)  of  the  dissolved  gas 
is  not  reduced  to  o°  and  760  mm.  The  solubility  /  is  therefore  the  volume 
of  gas  dissolved  by  unit  volume  of  the  solvent  at  the  temperature  of  the 
experiment.  The  two  expressions  are  related  thus: 


+0.00367    I), 


SOLUBILITY  IN  WATER  AT  PRESSURES  ABOVE  ONE  ATMOSPHERE. 

(Wroblewski  —  Compt.  rend.  94,  1335,  '82.) 

.Pressure    Coefficient  of  Saturation  *  at  : 
in  Atmos-    .  -  *  -  . 
pheres.  I2-4  • 


Pressure*     Coefficient  of  Saturation  *  at: 
in  Atmos-      /  -  *  -  > 


pheres. 

i 

5 
10 


1-797 
8.65 
16.03 


I2-4  • 

i.  086 
5.15 

9-65 


20 
25 
30 


21.65 
30.55 
33-74 


17.11 
20.31 
23.25 


*  Coefficient  of  Absorption  is  no  doubt  intended. 

SOLUBILITY  OF  CO2   IN  AQUEOUS   SOLUTIONS  OF  ACIDS   AND   SALTS 

(Geffcken.) 


Aq. 

Gms.  Acid 

CO2  Dissolved,  /  at: 

Aq. 

Gms. 

Salt 

C( 

D2  Diss 

olved,  I  at 

Solvent. 

per  Liter. 

15°. 

25°  •  ' 

Solvent. 

per  Liter. 

15°. 

25°-' 

HC1 

18.23 

I 

•043 

0 

.806 

CsCl 

84 

•17 

i 

•  006 

0.781 

ti 

36.46 

I 

.028 

0 

•799 

KC1 

37 

•30 

o 

.976 

0-759 

tt 

72.92 

I 

.000 

0 

•795 

KC1 

74 

.60 

o 

.897 

0.700 

HNO3 

3I-52 

I 

.078 

0 

.840 

KI 

83 

.06 

o 

992 

o-775 

« 

63-05 

I 

.086 

0 

•853 

KI 

166 

.12 

0 

923 

0.727 

tt 

126.10 

I 

.100 

0 

.877 

KBr 

59 

•55 

o 

.986 

0.768 

H,so4 

24.52 

I 

.018 

0 

•794 

KBr 

119 

.11 

o 

.914 

0.713 

« 

49.04 

O 

.978 

0 

.770 

KNO3 

5o 

•59 

I 

•005 

0.784 

tt 

98.08 

O 

.917 

0 

•730 

KN03 

101 

.19 

0 

.946 

0-749 

ti 

I47-II 

0 

.870 

0 

.698 

RbCl 

60 

•47 

o 

.989 

0.769 

tt 

196.15 

o 

.828 

0 

.667 

RbCl 

1  20 

•95 

o 

.921 

0.788 

CARBON    DIOXIDE 


106 


SOLUBILITY  IN  AQUEOUS 

SOLUTIONS  OP  SALTS. 

(Mackenzie  —  Wied.  Ann.  Physik.[2]  i,  450,  '77.) 

Salt  in 
Solution. 

Gms.  Salt  per                Density  of 
loo  Gms.  Solution.        Solution  15°. 

Absorption  Coefficient  a  at: 

8°.                               15°.             22°? 

KC1 

6.05                    I.  021 

0.988               0.777    0.670 

" 

8.646                 1.053 

0.918               0.777    0.649 

" 

11-974                 I.oSo 

0.864               0.720    0.597 

" 

22.506            1-549 

0.688               0.571     0.480 

NaCl 

7.062             1-038 

0.899(6.4°)     0.735 

tt 

12.995             1-080 

0.633(6.4°)     0.557    0.482 

tt 

17.42              1.123 

0.518(6.4°)     0.431     0.389 

tt 

26.00 

•195 

0-347(6-4°)     0.297     0.263 

NH4C1 

6.465 

.021 

1.023                0-825     0.718 

tt 

8.723 

•047 

i.ooo                0-791     0.702 

" 

12.727 

•053 

0.922                0.798    0.684 

'•' 

24-233 

.072 

0.813  (10°)       0.738    0.600 

8°.                     l6.5°.                    22°.                       30°. 

BaCLj 

7.316 

.068 

0.969          0-744          0.680          0.566 

i( 

9-753 

.092 

1.  02  1       0.645       0-607       0.543 

tt 

14.030 

•137 

0.618     0.524    0.467 

11 

25-215 

•273 

0.495     0.618     0.383     0.315 

SrC^ 

9-511 

.087 

0.779     0.663     0.581     0.508 

tt 

12-325 

•1159 

0.737     0.586    0.507     0.539 

tt 

I7-7I3 

.173 

0.606    0.473     0.444    0-367 

11 

31  .194 

•343 

0.285     0.245     0.247     0.223 

CaCl, 

4-365 

.036 

0.942     0.759    0.673     0.596 

1C 

5-739 

.049 

0-855     0.726     0.616    0.527 

tt 

8.045 

.068 

0-838    0.674    0.581     0.500 

It 

15-793            i-i39 

0-632     0.520    0.471     0.400 

SOLUBILITY  OP  CARBON  DIOXIDE  IN  ALCOHOL. 

(Bohr  — Wied.  Ann.  Physik  [4]  i,  247,  Joo.) 

In  99  per  cent  Alcohol.  In  98.7  per  cent  Alcohol. 

t0         cc.  CO2  (at  o°  and  760  mm.)  per  i  cc.      cc.  CO2  (at  o°  and  760  mm.)  per  i  cc. 


Alcohol.       Sat.  Solution. 

Alcohol.       Sat.  Solution. 

-65 

38.41 

35-93 

39.89 

37-22 

—  20 

7-5i 

7.41 

7-25 

7.16 

—  10 

5-75 

5-69 

5-43 

5-38 

O 

4-44 

4.40 

4-35 

4-31 

+  10 

3-57 

3-55 

20 

2.98 

2.96 

.  .  . 

25 

2  .76 

2-74 

.  .  . 

30 

2-57 

2.56 

40 

2  .20 

2  .19 

45 

2.OI 

2.00 

icy 


CARBON    DIOXIDE 


SOLUBILITY  IN  AQUEOUS  ALCOHOL  AT  20°. 

(Miiller  —  Wied.  Ann.  Physik.  [2]  37,  39.  '89;  Lubarsch  —  Ibid.  [2]  37.  525,  '89.) 


Density  of 

Per  cent  Alec 

Alcohol. 

By  Wt. 

0.998 

1.07 

0.969 

22.76 

0-960  (22 

•4°) 

28.46 

0-956 

3I-I7 

tt>s.  Coef. 

Density  of            Per  cent  Alcohol  Abs.  Coef. 

)f  CO2,  a. 

Alcohol. 

By  Wt. 

Of  C02,  a. 

0.861 

0.922 

49-o 

0.982 

0.841 

0.870(18.8°) 

71.1 

1.293 

0.792 

0.835(16°) 

85-3 

1.974 

O.Sol 

o-795  to0) 

99-7 

2.719 

0.877 

42.15 


SOLUBILITY  OF  CARBON  DIOXIDE  IN  ORGANIC  SOLVENTS. 

(Just  — Z.  physik.  Chem.  37,  354.  '01.) 


Solvent. 


Sol.  of  CO2,  Ostwald  Expression." 


CS2 

C.H.NH, 

C5HnOH 

C6H5Br 

CC14 

C.H.CH, 

CXN02 


0.870 
1.324 
1.831 
1.842 
2.294 

2-305 
2.425 
2.456 


0.889 

1-434 
1.941 
1.964 

2.502 

2  .426 
2.540 
2-655 


Q-945 
i-53i 

2.058 

2  .092 
2.603 

2-557 
2.716 

2.845 


Solvent. 

C3H7OH 

C2H5OH(95%) 

C6H5COH 

CHC13 

CH3OH 

CH3COOH 

(CH3CO)20 

(CH3)2CO 


Sol.  of  CO2,  Ostwald  Expression* 


fee- 
2.498 
2.706 
2.841 
3-430 

4.691 

5  .206 
6.295 

ho. 

2.923 

3-057 
3.681 

4.205 
5.129 
5.720 

6.921 

3-130 
3-304 

4.606 
5.614 
6.18 

*  See  p.  105. 


Determinations  are  also  given  for  the  solubility  in  glycerine,  iod 
benzene,  o  and  m  toluidine,  eugenol,  benzene  tri  chloride,  cumol, 
carvene,  di  chlor  hydrine,  iso  butyl  alcohol,  benzyl  chloride,  meta  xylol, 
ethylene  bromide,  chlor  benzene,  propylene  bromide,  amyl  bromide, 
carvol,  amyl  chloride,  iso  butyl  chloride,  butyric  acid,  ethylene  chloride, 
pyridine,  amyl  formate,  propionic  acid,  amyl  acetate,  iso  butyl 
acetate,  and  in  methyl  acetate. 

See  Woukoloff  —  Compt.  rend.  108,  674;  109,  62,  '89,  for  the  solubility 
of  CO2  in  CS2  and  CHC13  at  different  pressures. 


CARBON    MONOXIDE    CO. 

SOLUBILITY  IN  WATER. 

(Winkler  —  Ber.  34,  1416,  *oi.) 


to 

|3,  "Absorp 

1 

3',  "  Solu- 

o 

/3,  "Absorp. 

/ 

V,  "Solu- 

. 

Coef." 

bility." 

Q- 

I 

Coef." 

bility." 

'• 

o 

0 

•03537 

O 

•03516 

0 

.0044 

40 

0.01775 

O 

.01647 

O-OO2I 

5 

0 

•03149 

O 

.O3I22 

O 

•0039 

50 

O.Ol6l5 

O 

.OI42O 

O-OOlS 

10 

0 

.028l6 

o 

.02782 

o 

•0035 

60 

0.01488 

0 

-OII97 

O.OOI5 

15 

0 

•02543 

o 

.02501 

o 

.0031 

70 

O.OI44O 

o 

.00998 

O.OOI3 

20 

o 

.02319 

o 

.O2266 

o 

.0028 

80 

O.OI43O 

o 

.00762 

O-OOIO 

25 

0 

.O2I42 

o 

.02076 

0 

.OO26 

90 

O.OI42O 

o 

.  00438 

0.0006 

0 

.01998 

o 

.01915 

o 

.OO24 

100 

O.OI4IO 

0 

.00000 

o-oooo 

/8  =  vol.  of  CO  absorbed  by  i  volume  of  the  liquid  at  a  partial  pres- 
sure of  760  mm.  See  page  105. 

ft'  =  vol.  of  CO  (reduced  to  o°  and  760  mm.)  absorbed  by  i  volume 
of  the  liquid  under  a  total  pressure  of  760  mm. 

q  =  grams  of  CO  dissolved  by  100  grams  H2O  at  a  total  pressure  of 
760  mm. 


CARBON    MONOXIDE 


1 08 


SOLUBILITY  OF  CARBON  MONOXIDE  IN  AQUEOUS  ALCOHOL  SOLUTIONS 
AT  20°  AND  760  MM.  PRESSURE. 

(Lubarsch  —  Wied.  Annalen  Physik.  [2]  37,  525.  '89-) 
Wt.%  Alcohol.    Vol.%  Absorbed  CO.    Wt.  %  Alcohol.    Vol. %  Absorbed  CO. 

o.oo  2.41  28.57  1.50 

9-09  J-87  33-33  !-94 

16.67  J-7S  50.00  3.20 

23.08  1.68 


SOLUBILITY  OF  CARBON  MONOXIDE  IN  ORGANIC  SOLVENTS. 

(Just  —  Z.  physik.  Chem.  37,  361,  *oi.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression,  see  p.  105. 

Solvent. 

Water 

Anilin 

Carbon  Bisulphide 

Nitro  Benzene 

Benzene 

Acetic  Acid 

Amyl  Alcohol 

Xylene 

loo  volumes  of  petroleum  absorb  12.3  vols.  CO  at  20°,  and  13.4  vols» 
at  10°. 

(Guiewaszr  and  Walfisz  —  Z.  physik.  Chem.  i,  70,  '87.) 


/25. 
O.O24O4 

0.08314 
0.09366 
0.1707 
O.I7I4 
O.I7I4 
O.I78I 

0.02586 
0.05055 

o.  08112 
0.09105 
o.  1645 
o.  1689 
o.  1706 

0.1744 

Solvent. 

Toluene 
Ethyl  Alcohol 
Chloroform 
Methyl  Alcohol 
Amylacetate 
Acetone 
Iso  Butyl  Acetate 
Ethyl  Acetate 

te. 
0.1808 
o.  1921 
0.1954 

0.2140 
0.2225 
0.2365 
0.2516 

0.1742 
o.  1901 

0.1897 

o.  1830 
0.2108 
0.2128 

0.2314 

0.2419 

SOLUBILITY  OF  CARBON  MONOXIDE  IN  MIXTURES  OF  ACETIC  ACID  AND 
OTHER  SOLVENTS  AT  25°. 

(Skirrow  —  Z.  physik.  Chem.  41,  148,  '02.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression,  see  p.  105. 


Mixture  of 
Acetic  Ac.  and: 

%  CHgCOOH 
in  Mixture. 

CO. 

By  Wt. 

By  Vol. 

Anilin 

IOO.O 

IOO.O 

0.173 

" 

86.5 

90.8 

O.I  10 

« 

58.3 

68-5 

0.070 

" 

13-8 

25.1 

0.058 

tt 

O-O 

o.o 

0-053 

Benzene 

67-5 

63-4 

0.199 

" 

33-6 

29.6 

0.198 

" 

19.2 

16.5 

0.190 

n 

o.o 

o.o 

0.174 

Mixture  of 
Acetic  Ac.  and  : 

Chloroform 
tt 

Nitro  Benzene 
tt 

Toluene 
ft 

%  CH3COOH 
in  Mixture. 

CO. 

/25- 

0.196 
0.206 

0.156 
0.130 
0.093 

0.191 

0.195 

0.190 

0.182 

ByWt.      By  Vof. 
56.4      64.5 
0-0         0-0 
88.4      84.8 

49.0     66.3 
o-o       o-o 

74.7    71.0 

56.9     52.6 
20.5     17.8 
o.o      o-o 

109 


CARBON    MONOXIDE 


SOLUBILITY  OF  CARBON  MONOXIDE  IN  MIXTURES  OF  ACETONE  AND 
•OTHER  SOLVENTS  AT  25°. 

(Skirrow.) 


Mixture  of         %(CH3)2 

CO  in  Mixture.  CO. 

Mixture  of 

%(CH3)2CO  in 
Mixture. 

CO. 

Acetone  and: 

By  Wt. 

By  Vol. 

Acetone  and: 

By  Wt. 

By  Vol. 

IK- 

Anilin 

IOO. 

0 

IOO.O 

0. 

238 

Chloroform 

66. 

6 

78. 

9 

0.226 

" 

79- 

2 

85-9 

0. 

179 

" 

26. 

5 

40. 

4 

0.212 

" 

44- 

9 

56.7 

0. 

no 

" 

0. 

o 

O. 

o 

0.207 

"                                                0.0 

0.0 

0. 

053 

8  Naphthol 

86. 

0 

93- 

9 

o.  190 

Carbon  Bisulphide 

82. 

0 

83.8 

0. 

236 

ti 

73- 

I 

87- 

i 

o.  169 

" 

50. 

5 

61.8 

0. 

227 

Nitro  Benzene 

78- 

4 

88. 

5 

0.207 

it 

26. 

o 

35-7 

o. 

187 

" 

46. 

8 

69. 

5 

0-157 

ft 

14- 

5 

21.2 

0. 

144 

(I 

0. 

0 

0. 

o 

0.090 

" 

o. 

o 

O.O 

o. 

096 

Phenanthrene 

87- 

2 

95- 

4 

o.  205 

Naphthalene 

86. 

7 

93-5 

0. 

199 

" 

75- 

0 

90. 

2 

0.183 

" 

72. 

6 

85-4 

o. 

187 

SOLUBILITY  OF  CARBON  MONOXIDE  IN  MIXTURES  OF  BENZENE  AND 
OTHER  SOLVENTS  AT  25°. 

(Skirrow  —  Z.  physik.  Chem.  41,  144,  '02.) 

The  solubility  of  the  CO  given  in  terms  of  the  Ostwald  Expression, 
see  p.  105. 


Mixture  of 
Benzene  and: 

Naphthalene 


Phenanthrene 
a  Naphthalene 
Ethyl  Alcohol 


%CeH6  in 
Mixture. 


By  Wt. 

IOO.O 

88.5 

66.2 
89.2 
72.6 

96.5 
87.9 

47-7 
o.o 


By  Vol. 

IOO.O 
92.6 
76.3 

95-i 
85.8 
98.1 
93-i 
44-9 
o.o 


CO. 

/25- 
0.174 

o.  164 
o.  141 
0.144 
0.127 
0.149 
0.139 
0.181 

0.192 


Mixture  of 
Benzene  and: 


Anilin 


Nitro  Benzene 


%C6H6  in 
Mixture. 

'ByWt.'~ 
87.3 

71. 7 
42.6 

21.  2 


0.0 
71.8 

45-1 
o.o 


By  Vol. 
89.I 

75-2 
47.0 

24.3 
o.o 

80. 1 

56-4 
o.o 


CO. 

/25. 

o.  156 

0.131 
0.095 
0.068 

°-°53 
o.  152 
o.  127 

0.093 


SOLUBILITY  OF  CARBON  MONOXIDE  IN  MIXTURES  OF  TOLUENE  AND 


OTHER  SOLVENTS  AT 

(Skirrow.) 


25 


Mixture  of 
Toluene  and: 

%QH5CH3  in 
Mixture. 

CO. 

/25- 

Mixture  of 
Toluene  and: 

%C6H5CH3in 
Mixture. 

CO. 

126- 

B'y  Wt. 

By  Vol. 

By  Wt. 

By  Vol. 

Anilin 

IOO 

.0 

IOO.O 

0 

.182 

a  Naphthol 

95-5 

97 

.1 

O.I7I 

« 

94 

•4 

93 

•5 

0 

169 

a 

91.2 

94 

.2 

O.l62 

tl 

80 

.1 

80 

•3 

o 

,148 

Nitro  Benzene 

81.7 

85 

-7 

0.160 

tl 

55 

•4 

55 

.6 

0 

•"5 

tt 

50.8 

58 

.1 

0.131 

tt 

25 

•4 

25 

.6 

o 

,077 

(( 

23-7 

29-3 

0.108 

tl 

0 

.0 

0 

.0 

o 

053 

ti 

O-O 

o 

.0 

0.093 

Naphthalene 

92 

•9 

94 

.8 

o 

.169 

Phenanthrene 

94-4 

97 

.0 

0.170 

tt 

84 

•9 

88 

•7 

0 

.161 

it 

88.8 

93 

•9 

o.  161 

tt 

77 

•3 

82 

•5 

0 

•153 

it 

78.4 

87 

•5 

0.147 

CARBON    MONOXIDE  no 

SOLUBILITY  OF    CARBON  MONOXIDE    IN   MIXTURES  OF  ORGANIC 
SOLVENTS  AT  25°. 

(Skirrow.) 

%  of  Latter  in  Mixture.        CO 

Mixture  Composed  of:                                                     By  Wt.   '     By  Vol.  fa.  ' 

Chloroform  and  Methyl  Alcohol                           o.o  o . 207 

"                                                                    13.0  0.202 

"                                   "                              100  0.196 

Carbon  Bisulphide  and  Ethyl  Di  Chloride                       100  0.147 

75  0.157 

51  0.160 

"                 18.4  0.140 

o.o  0.083 

Methyl  Alcohol  and  Glycerine                              o.o          o.o  0.196 

39.6        30.1  0.096 

60.5         50.1  0.052 

77.1        68.9  0.025 

"                            "                                     100.0       100.0  very  small 

NOTE.  —  From  the  results  shown  in  the  preceding  five  tables,  it  is 
concluded  that  the  solubility  of  carbon  monoxide  in  various  mixtures 
of  organic  solvents  is,  in  general,  an  additive  function. 


CARBON    BISULPHIDE    CS2. 

SOLUBILITY  IN  WATER. 

(Chancel  and  Parmentier  —  Compt.  rend.  loo,  773,  85;  Rex  —  Z.  physik.  Chem.  55,  355,  '06.) 

Grams  CS2  per  100  Grams  CS2  pe'  100 

*°-        cc.  Solu-         Cms.  H2O'  t  °.  cc.  Solu-         Gms.  H2O 

tion.  (Rex).  tion.  (Rex). 

o  0.204  0.258        30  0.155    0.195 

5  0.199  35  0.137 

10  0.194  0.239        40  o.i  ii 

15  0.187  45  0.070 

20  0.179  o.ioi        49  0.014 

25  0.169 

100  cc.  H2O  dissolve  o.i  74  cc.  CS2  at  22°;  Vol.  of  solution=  100.208, 
Sp.  Gr.  =  0.9981. 

100  cc.  CS2  dissolve  0.961  cc.  H2O  at  22°;  Vol.  of  solution=  100.961, 

Sp.  Gr.  =    1.253.  (Herz  —  Ber.  31,  2670,  '98.) 

SOLUBILITY  OF  CARBON  BISULPHIDE  IN: 
Aq.  Solutions  of  Ethyl  Alcohol  at  17°.  Methyl  Alcohol. 

(Tuchschmidt  and  Folleuins  —  Ber.  4,  583,  '71.)  (Rothmund  —  Z.  physik.  Chem.  26,  475,  '08.) 

Wt.  per          Gms.  CS2  Wt.  per    Gms.  CS2  Wt.  per  cent  CS2  in: 


cent  per  100  cc.  cent         per  100  cc.  t  °.  pij,OH  pc0  ' 

Alcohol.  Solvent.  Alcohol.        Solvent.  "  Layer. 


ioo      oo      9!-37    5o       10       45.1  98.3 

98-5       l82        84.12     30          20           50.8  97.2 

98.15      132        76.02     20          25           54.2  96.4 

96.95     IOO        48.40      2          30           58.4  95.5 

93-54          7o            47-90          o               35                 64.0  93.5 

40  .  5  (crit.  temp.  )  80  .  5 


Ill 


CARBON    OXYSULPHIDE 


SOLUBILITY  OF  CARBON  OXYSULPHIDE  IN  WATER. 

(Winkler;  see  Landolt  and  Bernstein's  Tabellen,  ad  ed.  p.  602,  1906.) 


o 

5 

IO 
I5 


1-333 

1-056 
0.835 
0.677 


t°. 

20 

25 
3O 


8. 

o-56i 

0.468 
0.403 


0.356 

0.28l 
O.22I 
0.179 

For  ft  and  q  see  Carbon  Dioxide,  page  105. 
CARBON  TETRACHLORIDE.     Seep.  201. 
CARVOXIME    C10H4:NOH. 

SOLUBILITY  IN  r  LIMONENE. 

(Goldschmidt  and  Cooper  —  Z.  physik.  Chem.  26,  714,  '98.) 


q. 

0.147 

0.122 
O.IO4 


Gms.  C10H4:NOH 

Gms.  C10H4:NOI 

I 

t°.           per  100  Gms.          Solid  Phase. 

t  °.          per  100  Gms. 

Solid  Phase. 

r  Limonene. 

r  Limonene. 

24.6           44-6         /  Carvoxime 

48                  198.7 

/  Carvoxime 

30.0          59.2         /  Carvoxime 

49-4         199-7 

r  Carvoxime 

30.3          °3-3         r  Carvoxime 

55-4        325-1 

/  Carvoxime 

38.4         104.3         /Carvoxime 

55-9        346.6 

r  Carvoxime 

39  .  4         103  .  i         r  Carvoxime 

58.8        560.0 

r  Carvoxime 

43.1         130.8        /Carvoxime 

63.2         126.93 

r  Carvoxime 

CERIUM    ACETATE,  BUTYRATE,  FORMATE,  etc. 
SOLUBILITY  IN  WATER. 

(Wolff  —  Z.  anorg.  Chem.  45,  102,  '05.) 

Grams  Anhydrous  Salt  per  100  Gms.  Solution  at: 


Salt. 

Acetate 
Butyrate 
Iso  Butyrate 
Formate 
Propionate 


Formula. 


Ce(C2H302)3.iiH20 
Ce(C4H702)3,  and3H20 
Ce(C4H702)3.3H20 
Ce(CH02)8 
Ce(C3H502)3.H20,  and  3H2O 


3-544 


15°- 
19.61 

3.406 
6.603(20.4°) 

0.398(13°) 
18.99 

76°. 
12.97 
1.984 

3-39 
o.374(75-30) 
15-93 

CERIUM    AMMONIUM    NITRATE    (Ceri)   Ce(NO3)4.2NH4NO3. 
SOLUBILITY  IN  WATER. 

(Wolff.) 


te. 

Gms.  per  100  Gms. 
Solution. 

Atomic 
Relation. 

Gms.  Ce(N03)4-2NH4N03 
per  100  Gms. 

25 

4 

NHU. 
.065 

15 

Ce. 

16 

NH* 

2.08 

:       Ce. 

I 

Solution. 

Water. 
140.9 

35-2 

4 

•273 

16 

10 

2 

.06 

I 

61.79 

161  .7 

45-3 

4 

.489 

16 

69 

2 

.08 

I 

64.51 

174.9 

64-5 

4 

.625 

(IS 

40  Ce 
03  Ce 

IV 

2 
2 

.06 
•39 

i  Ce 
iCe 

IV 

66.84 

201  .6 

85.6 

4 

.778 

|x8. 

Us- 

i6Ce 
79  Ce 

IV 

2 
2 

04 

34 

iCe 
i  Ce 

IV 

69.40 

226.8 

(22. 

82  Ce 

2 

08 

iCe 

112 

.117 

|i6. 

22  Ce 

IV 

2 

95 

iCe 

IV 

88.03 

735-4 

CERIUM  AMMONIUM  NITRATE      112 

CERIUM  AMMONIUM  NITRATE    (Cero)  Ce(NO3)3.2NH4NO3.4H2O. 
SOLUBILITY  IN  WATER. 

(Wolff.) 


Gms.  per  100  Gms. 
to                   Solution. 

Atomic  Relation. 

per  100  Gms. 

NH4. 

Ce.     " 

NH4 

Solution. 

Water.' 

8 

75 

4 

.787 

18 

•56 

I 

•999 

I 

70 

.2 

235-5 

25 

o 

5 

.09 

19 

.80 

I 

•995 

I 

74 

.8 

296.8 

45 

o 

5 

•53 

21 

.06 

2 

•037 

I 

80 

•4 

410-2 

60 

0 

6 

.01 

22 

•77 

2 

•054 

I 

87 

.2 

681.2 

65 

06 

6 

.11 

23 

.42 

2 

.022 

I 

89 

.1 

817.4 

CERIUM    AMMONIUM    SULPHATE    Ce2(SO4)3.(NH4)2SO4.8H2O. 
SOLUBILITY  IN  WATER. 

(Wolff.) 


t°.  c 

Gms. 
per  100  G 

I4)2SO4         Solid 
ms-              Phase. 

Gms. 
.0       Ce2(S04)3.(NH4)2S04 
1   •             per  100  Gms. 

Solid 
Phase. 

Solution. 

Water". 

Solution. 

Water. 

22.3 

5 

.06 

5 

33         -8H20 

45 

.0 

2 

-91 

2 

99 

Anhydride 

35  -1 

4 

•93 

5 

.18 

55 

•25 

2 

.16 

2 

.21 

ii 

45-2 

4 

.76 

4 

•99 

75 

•4 

I 

.46 

j 

,48 

11 

85 

.2 

I 

•17 

j 

.18 

" 

CERIUM    SULPHATE    Ce2(SO4)3. 

SOLUBILITY  OP  THE  SEVERAL  HYDRATES  IN  WATER. 

(Koppel  —  Z.  anorg.  Chem.  41,  377,  '04;  the  previous  determinations  by  Muthman  and  Rolig  —  Z. 
anorg.  Chem.  16,  455,  '98,  and  by  Wyrouboff  —  Bull.  soc.  chim.  [3]  25,  121,  '01,  are  shown  by  Koppel 
to  be  inaccurate.) 


Gms. 


Solution. 


o 

14.20 

0-525 

18.8 

14.91 

o-555 

19.2 

15.04 

0.561 

o 

17  .35 

0.665 

IS 

10.61 

0-376 

21 

8.863 

0.308 

31.6 

6.686 

0.227 

45-6 

4.910 

0.164 

5° 

4-465 

0.148 

60 

3-73 

0.123 

65 

3-47 

0.114 

o 

*5-95 

0.605 

15 

9-95 

o-35o 

Solid  Phase. 


Ce2(SO4)3.i2H2O 


Ce2(SO4)3.gH2O 


Ce2(S04)3.8H20 


Gms. 


Mols 


Gms. 

wo 

Solution. 

2    ' 

20.5 

8.69 

0.302 

40 

5-6I3 

0.188 

60 

3.88 

0.129 

45 

8.II6 

0.280 

60 

3-145 

0-103 

80 

I.I9 

0.0382 

100.5 

0.46 

0.0149 

35 

7-8 

0.27 

40 

5-7i 

0.19 

5° 

3-3i 

O.II 

65 

1-85 

0.06 

82 

0.98 

0.032 

100.5 

0.42 

0.014 

Solid  Phase. 


Ce2(S04)3.8H20 


Ce2(S04)3.5H20 


Ce2(S04)3.4H2O 


H3  CHLORAL    HYDRATE 

CHLORAL    HYDRATE   C2HC13O.H2O. 

SOLUBILITY  IN  WATER,  ETHYL  ALCOHOL,  CHLOROFORM,  AND  IN 

TOLUENE. 

(Speyers  —  Am.  J.  Sci.  [4]  I4t  294,  '02.) 

Calculated  from  the  original  results,  which  are  given  in  terms  of 
gram  molecules  of  chloral  hydrate  per  100  gram  mols.  of  solvent. 


In  Water. 

In  Alcohol. 

In  Chloroform. 

In   Toluene. 

W.                   S. 

'W.               S.  ' 

W.                   S. 

w.            s: 

o     1.433     l89-7 

I.  11    123.3       I 

•530        3-7 

0.898           3.2 

5     1.460    233.0 

1.16     130.0        i 

•5*5        4-o 

0.900           4-O 

10     1-485     275.0 

.23     140.0        i 

.510        5.0 

0.910            7.0 

15     1.510    330.0 

.30     160.0         i 

.505        9.0 

0.915       ii.  o 

20       1-535       383.0 

.36     185.0         i 

.510      19.0 

0-94            21.0 

25     1-555     433-o 

.42     215.0         i 

.520      34.0 

o-97        36-° 

30     1.580    480.0 

•49     245.0         i 

.540      56.0 

i.  02        56.0 

35     1.59       516.0 

.55     280.0        i 

.570      80.0 

1.13        80.0 

40     i  .  605 

i.  60    320.0        i 

.590     no.o 

1.40       no.o 

45     i  .620 

... 





W  =  wt.  of   i  cc 

.   saturated  solution 

,  S  =  Gms.  C2 

HC13.H2O  per  100 

grams  solvent. 

CHLORINE    Cl. 

SOLUBILITY  IN 

WATER. 

(Winkler  —  Landolt  and  Bernstein's  Tabellen,  sd  ed.  p. 

532,  60  1,  '06;   Roozeboom  —  Rec.  trav.  chlm, 

3* 

59,  '84;  4,  69,  '85;  Z.  physik. 

Chem.  2,  452,  '88.) 

to                       or 

n                                           *•  ° 

Gms.  Cl  per 

Solid 

P  • 

q.                            c    . 

loo  Gms.  H2O. 

Phase. 

o        4.610 

1.46                    —O.24 

0.492 

Ice+C1.8aq. 

3        3-947 

1.25                   o 

0.507-0.560 

C1.8  aq. 

6        3.411 

1.  08                          2 

0.644 

it 

9        3-031 

0.96                   4 

0.732 

« 

9.6       2  .  980 

0.94                  6 

0-823 

« 

12.  O       2.778 

0.88                  8 

0.917 

« 

10         3.095 

0.997                9 

o  .  965-0  .  908 

K 

15             2  -635 

0.849              20 

i.8S 

it 

2O            2.26o 

0.729              28.7 

3-69 

« 

25                -985 

0.641 

30                .769 

0.572 

40            .414 

0-459 

50            .204 

o-393 

60            .  006 

0.329 

70         0.848 

0.279 

80         0.672 

0.223 

90         0.380 

0.127 

IOO            O-OOO 

0-000 

p'  =  vol.  of  Cl  (red.  to  o°  and  760  mm.)  absorbed  by  i  vol.  H2O  at 
total  pressure  of  760  mm. 

q  =  Gms.  Cl  per  100  gms.  H2O  at  a  total  pressure  of  760  mm. 


CHLORINE  114 

SOLUBILITY  IN  WATER. 

(Goodwin  —  Ber.  15,  3039,  '82.) 

The  saturated  aqueous  solution  of  the  chlorine  was  cooled  until 
chlorhydrate  separated;  the  temperature  was  then  gradually  raised 
and  portions  withdrawn  for  analysis  at  intervals.  Slightly  different 
results  were  obtained  for  solutions  in  contact  with  much,  little,  or  no 
chlorhydrate.  The  following  results  are  taken  from  an  average 
curve. 

.o  Solubility  f0  Solubility  +  0  Solubility 

Coefficient.  Coefficient.  Coefficient. 

2-5  1.76  II  3-0  25  2.06 

5.0  2.00  12.5  2.75  30  1.8 

7.5  2.25  15  2.6  40  1.35 

10  2.7  20  2.3  50  i.o 

SOLUBILITY  OF  CHLORINE  IN  AQUEOUS  SOLUTIONS  OF  HYDROCHLORIC 
ACID  AND  OF  POTASSIUM  CHLORIDE. 

(Goodwin.) 
Coefficient  of  Solubility  in: 


t°. 

HC1 

HC1 

HCl 

KCl 

(1.046  Sp.  Gr.). 

(1.08  Sp.  Gr.). 

(1.125  Sp.  Gr.). 

(20  g.  per  loo  cc.). 

0 

4-1 

6.4 

7-3 

1.5 

5 

5-1 

5-2 

6.7 

2.0 

10 

4.1 

4-5 

6.1 

2.2 

15 

3-5 

3-9 

5-5 

1.6 

20 

3-o 

3-4 

4-7 

1.2 

25 

2-5 

3-o 

4.0 

1.0 

30 

2.0 

2.4 

0-9 

40 

1.25 

1.6 

Goodwin  also  gives  results  for  solutions  of  NaCl,  CaCl2,  MgCl2,  SrCl2, 
Fe2Cl2,  CoCl2,  NiCl2,  MnCl2,  CdCl2,  LiCl,  and  in  mixtures  of  some  of 
these,  but  the  concentrations  of  the  salt  solutions  are  not  stated. 

SOLUBILITY  OF  CHLORINE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

CHLORIDE. 

(Kumpf  —  Wied.  Ann.  Beibl.  6,  276,  '82;  Kohn  and  O'Brien  — J.  Soc.  Chem.  Ind.  17,  100,  '08.) 

Coefficient  of  Solubility  in: 


b 

9-97%  NaCl. 

i6.oi%NaCl. 

19.66%  NaCl. 

26.39%  * 

0 

2-3 

I.9 

J-7 

o-5 

5 

2.0 

1.6 

1.4 

0.44 

10 

i-7 

i-3 

I-IS 

0.4 

i5 

1.4 

i.  06 

o-95 

0.36 

20 

1.2 

0.9 

0.8 

0-34 

25 

0-94 

o-75 

0.65 

o-3 

50 

0.2 

80 

.  .  . 

.  .  . 

0.05 

TOO  cc.  of  6.2  per  cent  CaCl2  solution  dissolve  0.245  gram  Cl  at  12°. 
100  cc.  of  6.2  per  cent  MgCl2  solution  dissolve  0.233  gram  Cl  at  12°. 
100  cc.  of  6.2  per  cent  MnCl2  solution  dissolve  0.200  gram  Cl  at  12°. 

For  coefficient  of  solubility  see  page  105. 


ii5  CHLORINE    MONOXIDE 

CHLORINE    MONOXIDE    C12O. 

100  volumes  of  water  at  o°  absorb  200  volumes  of  C12O  gas. 

CHLORINE    TRIOXIDE    C12O3. 

SOLUBILITY  IN  WATER  AT  APPROX.  760  MM.  PRESSURE. 

(Brandan  —  Liebig's  Ann.  151,  340,  "69.) 
t°.  8.5°.  14.0°.  21°.  93°. 

Gms.  C12O3  per  ioo  gms.  H2O        4-765         5 -012         5-445         5-651 

Garzarolli  and  Thurnbalk — Liebig's  Ann.   209,  184,  '81,  say  that 
C12O3  does  not  exist,  and  above  figures  are  for  mixtures  of  C12O  and  Cl. 


CHLOROFORM    CHC13. 

SOLUBILITY  IN  WATER. 

(Chancel  and  Parmentier  —  Compt.  rend,  ioo,  473,  85;  Rex  —  Z.  physik.  Chem.  55,  355,  '06.) 

«.  o  Gms.  CHCla  per 

ioo  Gms.  H20  fcex). 

o  1.062 

10  0.895 

2O  O.822 

30  0.776 

ioo  cc.  H2O  dissolve  0.42  cc.  CHC13  at  22°;  Vol.  of  sol.  =  100.39  cc-» 
Sp.  Gr.  =  1.0002. 

ioo  cc.  CHC13  dissolve  0.152  cc.  H2O  at  22°;  Vol.  of  sol.  =  99.62  cc., 
Sp.  Gr.  =  1.4831. 

(Herz  —  Ber.  31,  2670,  '98.) 


t°. 

Gms.  CHC13  per 
Liter  of  Solution. 

Density 
of  Solutions. 

o 

9.87 

1.00378 

3-2 

8.90 

17.4 

7.12 

I  .00284 

29.4 

7-05 

1.00280 

41.6 

7.12 

I  .00284 

54-9 

7-75 

1.00309 

SOLUBILITY  OF  CHLOROFORM  IN  AQUEOUS  ETHYL  ALCOHOL,  METHYL 
ALCOHOL,  AND  ACETONE  MIXTURES  AT  20°. 

(Bancroft  —  Phys.  Rev.  3,  29,  '95,  '96.) 


:n  Ethyl 

Alcohol. 

In  Methyl  Alcohol. 

In  Acetone. 

Per  5  cc. 

C2H5OH. 

Per  5  cc. 

CH3OH. 

Per  5  cc. 

(CH3)2CO 

cc.  H20. 

cc.  CHC13. 

cc.  H2O. 

cc.  CHC13'. 

cc.  H2O. 

cc.  CHC13. 

10 

O.2O 

10 

O-IO 

5-o 

0.16 

8 

o-3 

5 

0.48 

4-0 

0-22 

6 

0-515 

4 

0.8o 

3-o 

o-33 

4 

1-13 

2 

4-0 

2  -O 

0.58 

2 

2.51 

1.49 

7-0 

I  -O 

o-955 

I 

4.60 

i-35 

8.0 

o-79 

I  .12 

0.91 

5-o 

I  .12 

IO.O 

0-505 

I.  60 

0.76 

6.0 

0.30 

2.50 

o-55 

8.0 

O-2I 

3-50 

0.425 

IO  -O 

0.19 

4-0 

0.2O 

20.  o 

0.16 

5-o 

0.125 

30.24 

0.12 

IO.O 

CHROMIUM    ALUMS  116 

SOLUBILITY  OF  CHROMIUM  ALUMS  IN  WATER  AT  25°. 

(Locke  — Am.  Ch.  J.  26,  174,  'ox.) 

Per  IPO  cc.  Water. 

Alum  Formula.  '  Grams          Grams Gram  ' 

Anhdyrous.  Hydrated.      Mols. 

Potassium  Chromium  Alum    KjCr^SO^^HjO     12.51     24.39    0.0441 
Tellurium  Chromium  Alum    TejCr^SO^^HjO    10.41     16.38    0.0212 

CHROMIUM    CHLORIDE    (ic)    CrCl3.6|H2O. 

100  grains  H2O  dissolve  130  grams  (green  modification)  at  15°. 

(Recoura  —  Compt.  rend.  102,  518,  '86.) 

CHROMIUM    DOUBLE    SALTS. 

SOLUBILITY  IN  WATER. 

(Jorgensen  —  J.  pr.  Chem.  [2]  20, 105,  '79;  [2]  30,  i,  '84;  [2]  42,  208,  '90;  Struve  —  Ibid.  [2]  61,  457, 

'990 

Gms.  per 

Name  of  Salt.  Formula.  t  °.     100  Gms. 

H20. 

Chloro     Tetra    Amine     Chromium 

Chloride  CrCl(NH3)4(OH2)Cl2  15  6.3 

Chloro  Purpureo  Chromium  Chloride  CrCl(NH3)5Cl2  16  0.65 

Luteo  Chromium  Nitrate  Cr(NH3)6(NO3)3       .  ?  2.6 

Chloro  Purpureo  Chromium  Nitrate  CrCl(NH3)6(NO3)2  17.5  1.4 

Chromic  Potassium  Molybdate  3K2O.Cr2O3.i2MoO3.2oH2O  17  2.5 

CHROMIUM    TRIOXIDE    CrO3. 

SOLUBILITY  IN  WATER. 

(Mylius  and  Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt,  3,  451,  'oo.) 


li 


Gms.  CrO3  per  100 
g.  Solution. 

Mols.  CrO3  per 
100  Mols.  H2O. 

Solid  Phase. 

62.08 

29.4 

CrOa 

62.38 

29.8 

(t 

62.45 

29.91 

" 

64.55 

32-7 

u 

50 

99  67.39  37 -1 

Density  of  solution  saturated  at  18°  =  1.705. 

CHROMIUM    SULPHATES    (ous  and  ic). 

SOLUBILITY  IN  WATER  (ous  at  o°). 

Salt.  G^5'  Pfjf  ^°°  Solid  Phase.  Authority. 

Lrins.  Jri2vJ. 

ChromOUS          12  .35        CrSO4.7H2O  (Moissan  —  Bull.  soc.  chim.  [2]  37,  296,  '82) 

Chromic          1 2O  .  O          Cr2(SOJ3. l8H2O     (Etard  —  Compt.  rend.  84,  1090,  '77.) 

CHRYSAROBIN   C30H26O7. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.) 
Solvent  Gms.  per  100  Gms.  Solvent  at;  Solvent  Gms.  per  100  Gms. 

Water  0.021         0-046  Chloroform  5.55 

Alcohol  0.324,       0.363  (60°)         Ether  0.873 

Benzene          4.0  ...  Amyl  Alcohol  3.33 

Carbon  Disulphide  o .  43 


ii7  GHRT8EN 

OHRYSEN   C18H12. 

SOLUBILITY  IN  TOLUENE  AND  IN  ABS.  ALCOHOL. 

(v.  Becchi.) 

ioo  gms.  toluene  dissolve  0.24  gm.  C18H,2  at  18°,  and  5.39  gms.  at 
100°. 

ioo  gms.  abs.  alcohol  dissolve  0.097  gm.  C18H12  at  16°,  and  0.170  gm. 
at  b.  pt. 

CINCHONA  ALKALOIDS.     (See  also  Quinine,  p.  269.) 
SOLUBILITY  or  CINCHONLNE,  CINCHONIDINE,  QUININE,  AND  QUINIDINE 
IN  SEVERAL  SOLVENTS  AT  i8°-22°. 

(Miiller  —  Apoth.-Ztg.  18,  233,  '03;  see  also  Prunier —  J.  pharm.  chim.  [4]  29,  136,  '79.) 

Grams  of  the  Alkaloid  per  ioo  Grams  Solution. 


Solvent. 

Cinchonine 

Cinchonidine 

CTJ      XT  /"» 

Quinine 
C20H24N20,. 

Quinidine 
r    H    M  O 

1»      22      2 

1< 

pU.g^A.^gVX* 

Hydrate. 

Anhydride. 

1^20^*  24™  2^2 

Ether 

O.IO 

0 

.211 

I 

619 

0 

.876 

o 

.776 

Ether  sat.  with  I^O 

0.123 

0 

•523 

5 

-6l8 

2 

•794 

I 

.629 

H2O  sat.  with  Ether 

0.025 

0 

.0306 

o 

.0667 

0 

.0847 

o 

•031 

Benzene 

0-0545 

0 

.099 

o 

.2054 

I 

.700 

2 

•451 

Chloroform 

0.6979 

9 

.301 

1  00  + 

100  + 

IOO  + 

Acetic  Ether 

0.0719 

0 

•3003 

4 

•65 

2 

.469 

I 

.761 

Petroleum  Ether 

0-0335 

0 

•0475 

o 

.0103 

0 

.0211 

0 

.0241 

Carbon  Tetra  Chloride  o  .0361 

0 

.0508 

o 

.203 

0 

•529 

o 

•565 

Water 

0.0239 

0 

•0255 

0 

•574 

0 

.0506 

o 

.0202 

Glycerine  (15  .5°) 

0.50 

o. 

50 

ioo  grams  chloroform  dissolve  0.565  gm.  cinchonine  at  50°. 
100  grams  abs.  ether  dissolve  0.264  gm.  cinchonidine  at  32°. 

(Kohler  —  Z.  anal.  Ch.  18,  242,  '79.) 


SOLUBILITY  or  CINCHONINE  AND  CINCHOTINE  SULPHATE,  TARTRATE, 

BlTARTRATE,    OXALATE,    AND    HYDROCHLORIDE    IN    WATER. 
(Forst  and  Bohringer —  Ber.  14,  1266,  '81.) 


Cinchonine  Salts. 


Formula. 


2(C19H22N20)S04H2.2H20      13 
2  (C19H22N2O)  C4H6O6_._2  H2O     1 6 

v^ioiioalN  o^-'  *^ 


2  (C19H02N2O)  .C2H4O4.H2O 
C19H22N2O.HC1.2H2O 


20 
10 


Gms.  per 

ioo  Gms. 

H2O. 


Cinchotine  Salts. 

Formula.  1 


1.52 
3.0 


2(C19H24N20)S04H2.2H20  13 

2(C19H24N20)C4H606.2H20  16 

C19H24N2O.C4H6O6.4H2O  1 6 

0.96     2  (C,9H24N2O)  .C2H2O4.H2O  10 

4.16     C19H24N2O.HC1.2H2O  10 


Gms.  per 

ioo  Gms. 

H2O. 

3.28 
I.76 
1.28 
1.16 

2.12 


SOLUBILITY  OF  CINCHONINE  SULPHATE   AND  OF  CINCHONIDINE   SUL- 
PHATE IN  SEVERAL  SOLVENTS. 


Solvent. 


(U.  S.  P.) 


Gms.  (C1 

per  ioo  Gms.  Solvent. 


At  25°. 

At  80°. 

Water 

1.72 

3-1 

Alcohol 

IO-O 

19.2(60°) 

Ether 

0.04 

.  .  . 

Chloroform 

i-45 

.  .  . 

Glycerine 

.6-7  (15°) 

Gms.  (C,«H22N20),.H2S04.3H20 
per  ioo  Gms.  Solvent. 


At  25°. 
1. 60 
1-4 
O-O2 
O.II 


At  80° 


(60°) 


CINNAMIC    ACID  118 

CINNAMIC    ACID    C6H5CH:CH.COOH. 

SOLUBILITY   OF   CINNAMIC   ACID  IN  AQUEOUS   SOLUTIONS  OF  SODIUM 
ACETATE,  BUTYRATE,  FORMATE,  AND  SALICYLATE  AT  26.4°. 

(Philip  — J.  Chem.  Soc.  87,  992,  '05.) 

Calculated  from  the  original  results,  which  are  given   in  terms  of 
molecular  quantities  per  liter. 


Cms.  Na  Salt 

Gms.  L 

6ii5UH:(JH.tJUUJtl  ] 

>er  Later  in  bolu 

-A. 

tions  of: 

per  Liter. 

CH3COONa. 

C3H7COONa. 

HCOONa. 

C6H4.OH.COO1 

0 

0.56 

0.56 

0.56 

0.56 

I 

1.50 

I.30 

0.92 

O.62 

2 

2.12 

I.8S 

I  .12 

0.70 

3 

2.52 

2  .25 

1.27 

o-73 

4 

2.85 

2.60 

I  .40 

0.77 

5 

3-05 

2-90 

1-47 

0.80 

8 

0.90 

i  liter  of  aqueous  solution  contains  0.491  gm.  C6H5CH:CH.COOH 
at  25°  (Paul). 

SOLUBILITY  OF  CINNAMIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ANILIN 
AND  OF  PARA  TOLUIDIN  AT  25°. 

(Lowenherz  —  Z.  physik.  Chem.  25,  394,  '98.) 

Original  results  in  terms  of  molecular  quantities  per  liter. 

In  Aqueous  Anilin.  In  Aqueous  p  Toluidin. 

Grams  per  Liter.  Grams  per  Liter. 


C6H5CH  :CHCOOH.  CeH^CHsNHa.    C6H5CH :  CHCOOH. 

0  0.49  o  0.49 

1  1. 2O  I  1.52 

2  1.65  2  2. 2O 

3  2.02  3  2.83 

4  2.35  4  3-35 
6                   2.92                          5  3.80 

SOLUBILITY   OF  CINNAMIC  ACID   IN  METHYL,   ETHYL,  AND  PROPYL 

ALCOHOLS. 

(Timofeiew  —  Compt.  rend.  112,  1137,  '91.) 

Grams  C6H5CH:CH.COOH  per  100  Grams  of: 
CH3OH.  C2H5OH.  C3H7OJL 

o  20.65  15-61  10.63 

19.5  28.91  22.03  IS-4I 

SOLUBILITY  OF  BROM  CINNAMIC  ACIDS. 

a  Brom  and  ft  Brom  Cinnamic  Acid     a  Brom  Cinnamic  Acid  in  Aq. 
in  Water  at  25°.  Solutions  of  Oxalic  Acid  at  25°. 

(Paul  —  Z.  physik.  Chem.  14,  in,  '94.)  (Noyes  —  Z.  physik.  Chem.  6,  245,  '90.) 

Per  loop  cc.  Solution.      Normality^ of  Solutions.      Grams  per  Liter. 

Acid-  Grams.    Millimols. '    (COOH)2.    C6H5CH:       (COOH)2.   C6H5CH: 

CBr:COOH.  CBrCOOH. 

a,  C6H5CH:  CBrCOOH     3.9325     17.32        o  0.0176    o.o          3.995 

/3,  C6H6CBr:  CHCOOH     0.5255      2.315      0.0275    0.0140    2.448      3.178 

0.0524  0.0129  4.716   2.928 


H9  CITRIC    ACID 

CITRIC    ACID    C3H4(OH)(COOH)3.H2O. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.;  Bourgoin  —  Ann.  chim.  phys.  [5]  13,  406,  '78.) 

Cms.  C3H4(OH)(COOH)3.H20  per  TOO  Cms. 

solvent .  t   .  » ,. 

Solution.  Solvent. 

Water  25  64.8  185 

Water  b.  pt.  70.3  250 

Alcohol  (90%)  25  34.6  75.9 

Alcohol  (U.S.P.)  39.2  64.5 

Alcohol  (Abs.)  "  43.2  52.8 

Ether  "  2.21                      2.26 

Ether  (U.S.P.)  5.2                        5.55 

COBALT    BROMIDE    CoBr2. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  537,  '94.) 


t°.                                                                59°.                75°. 

Gms.  CoBr2  per  100  gms.  solution          66.7        66.8 

COBALT    DOUBLE    SALTS. 

SOLUBILITY  IN  WATER. 

(Jorgensen  —  J.pr.  Chem.  [2]  18,  205,  '78;  19,  49,  '79;  Kurnakoff  —  J.  russ.  phys. 
'92.) 

Name.                                                   Formula. 

Chloro  purpureo  cobaltic  bromide     CoCl(NH3)5Br2 
Bromo  purpureo  cobaltic  bromide     CoBr(NH3)5Br., 
Chloro  tetra  amine  cobaltic  chloride  CoCl(NH3)4(OH8)Cl9 

97°. 

68.1  (blue) 

chem.  Ges.  24,  629, 

Gms.  Salt 
t°.          per  100 
Gms.  H2O. 

14.3         0.467 

16          0.19 
2.50 

Chloro  purpureo  cobaltic 

chloride 

CoCl(NH3)5Cl2 

0 

0.232 

Chloro  purpureo  cobaltic 

chloride 

CoCl(NH3)5Cl2 

15 

•5 

o 

.41 

Chloro  purpureo  cobaltic 

chloride 

CoCl(NH8)6CI2 

46 

6 

I 

•03 

Luteo  cobaltic  chloride 

Co(NH3)6Cl3 

o 

4 

.26 

Luteo  cobaltic  chloride 

Co(NH3)6Cl3 

46 

.6 

12 

•74 

Roseo  cobaltic  chloride 

Co(NH3)5(OH2)Cl3 

o 

16 

.12 

Roseo  cobaltic  chloride 

Co(NH3)5(OH2)Cl3 

16 

.2 

24 

.87 

Chloro  purpureo  cobaltic 
Chloro  purpureo  cobaltic 

iodide 
nitrate 

CoCl(NH3)5I2 
CoCl(NH3)5(N03)2 

J9 

15 

.2 

2 

I 

•  O 
•25 

Chloro  purpureo  cobaltic 

sulphate 

CoCl(NH3)5SO4.2H2O 

17 

•3 

0 

•75 

Nitrato  purpureo  cobaltic  nitrate 

Co(N03)(NH3)(N03)2 

16 

0 

•36 

COBALT    CHLORATE    Co(ClO3)2. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  35,  1419,  '02.) 


Gms.                Mols. 
to           Co(ClO3)2        Co(ClO3)2             Solid 
per  too  Gms.       per  100              Phase. 

Gms. 
to      Co(C103)2 
'  per  loo  Gms 

Mols. 
Co(C103)2             Solid 
per  loo               Phase. 

Solution. 

Mols.  H20. 

Solution. 

Mols. 

H20. 

—  12 

29 

•97 

o 

.41 

Ice 

18 

64 

.19 

14. 

28 

Co(C103)2.4H20. 

—  21 

53 

•3° 

9 

.08 

Co(ClO3)2.6H20 

.    21 

64 

•39 

14- 

51 

" 

—  19 

53 

.61 

9 

.20 

" 

35 

67, 

09 

16. 

10 

" 

O 

57 

•45 

10 

•75 

" 

47 

69, 

66 

18. 

29 

" 

10.5 

61 

12 

.90 

44 

61 

76 

.12 

25- 

39 

44 

Density 

of  solution  saturated  at 

18°  = 

I.86I. 

COBALT    CHLORIDE  120 

COBALT    CHLORIDE    CoCl2. 

SOLUBILITY  IN  WATER. 

(Etard  —  Compt.  rend.  113,  699,  '91;  Ann.  chim.  phys.  [7]  2,  537,  '94.) 

Gms.  Gms. 

«.„  CoCl2per  Solid  f0  CoCl2  per  Solid 

*   '          100  Gms.  Phase.  100  Gms.  Phase. 

Solution.  Solution. 

-io  27.0  CoCl2.6H2O  (red)         35  38.0    CoCl2.H2O  (violet) 

o  29.5  40  41.0 

H-io  •  31.5  50  47-o 

20  33-5  60  47.5     CoCl2.H20  (blue) 

25  34-5  8o  49-5 

30  35-5  I0°  5!-° 

SOLUBILITY  OP  COBALT  AMMONIUM  CHLORIDES  IN  WATER. 

(Kurnakoff  —  J.  russ.  phys.  chem.  Ges.  24,  629,  '93;  J,  Chem.  Soc.  64,  ii,  509,  '93.) 
.  Grams  per  100  Grams  H2O  at: 

o°^ 16.9°.  46.6°'. 

CoCl3.5NH3  0.232       ...         1.031 

CoCl^NHg-EL/)  16.12       24.87       ... 

CoCl3.6NH3  4.26         ...       12.74 

SOLUBILITY  OF  COBALT  CHLORIDE  IN  AQUEOUS  HYDROCHLORIC 
ACID  SOLUTIONS  AT  o°. 

(Engel  —  Ann.  chim.  phys.  [6]  7,  355,  '89.) 


Milligram  Mols. 
per  io  cc.  Sol.                        fp.J3r.rf 

Gms 

.  per  100  Gms. 
Solution. 

Gms.  per  100  cc. 

Solution. 

&CoCl2.            HCl. 

CoCl2. 

HCl. 

CoCl2. 

HCl. 

62 

-4 

0 

•343 

30 

•i7 

O 

.00 

40-5 

0 

58 

•52 

3 

•7 

-328 

28 

.62 

0 

.102 

38.0 

0 

•135 

50 

.8 

ii 

•45 

.299 

25 

•39 

0 

.321 

33-o 

0 

.417 

37 

•25 

25 

.2 

.248 

19 

•43 

0 

.738 

24.2 

0 

.919 

12 

•  O 

.167 

7-15 

I 

.718 

8-34 

2 

.00 

4 

•75 

74 

•75 

.150 

2 

.68 

2 

•369 

3-o8 

2 

•72 

12 

.0 

104 

•5 

.229 

6 

•34 

3 

.099 

7-79 

3 

.81 

25 

.0 

139 

•  o 

•323 

12 

•27 

3 

.829 

16.24 

5 

.07 

SOLUBILITY  OF  COBALT  CHLORIDE  IN  AQUEOUS  ALCOHOL 
AT   11.5°. 

(Bodtker  — Z.  physik.  Chem.  22,  509,  '97.) 

io  gms.  of  CoCl2.6H2O  were  added  to  20  cc.  of  alcohol  and  in  addition 
the  amounts  of  CoCl2  shown  in  the  second  column.  The  solutions  were 
shaken  2  hours,  5  cc.  withdrawn,  and  the  amount  of  dissolved  CoCl2 
determined  by  evaporation  and  weighing. 

Vol.  %     Gms.  CoCl2    Gms.  per  5  cc.  Solution.          Vol.  %     Gms.  CoCl2        Gms.  per  5  cc.  Sol. 
Alcohol.        Added.  H2O.          CoCl2.  Alcohol.      Added.  H2O.          CoCl2. 

91.3     o.o  1.325     1.168  99.3     0.612        0.764     1-459 

98.3     o.o  1-134     1-214  99.3     0.813         0.688     1.568 

98.3       0.0  1. 068       I.lSl  99-3       1-022  0.634       L7I3 

99.3     o.o  1.045     I-I99  99-3     I-24Q        0.553     i  831 

99.3     0.194        0.899     1.204  99-3     I-446        0.483     1.943 

99.3     0.400        0.829     1.325  99.3     1-650        0.500     2.183 

100  gms.  sat.  solution  in  alcohol  (0.792  Sp.  Gr.)  contain  23.66  gms. 

CoCla,  Sp.  Gr.  =    I.OI07.  (Winkler  —  J.pr.Chem.pi,  207, '64J 


121 


COBALT    CHLORIDE 


SOLUBILITY  OF  COBALT  CHLORIDE  IN  ORGANIC  SOLVENTS. 

Gms.  per  100  Gms.  Solvent. 


Solvent.  t°. 

Acetone  o 

"  22.5 

25 
18 
Ethyl  Acetate  14 

79 

Ether 
Glycol 

COBALT    IODATE    Co(IO3)2. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  34,  2435,  '01.) 
Solid  Phase  : 
t°.  Co(I03>.4H20.  Co(I03)2.2H20. 


CoCl2. 
9-II 
9.28 
8.62 

2-75 
0.08 
0.26 

0.021 


CoCl2.2H2o7  Authority. 

17.16    (St.  von  Laszczynski  —  Ber.  27,  2285,  '94.) 
1 7  •  06    (St.  von  Laszczynski  —  Ber.  27,  2285,  '94.) 
.  .  .       (Krug  and  McElroy  —  J.  Anal.  Ch. 6, 184/92.) 

(Naumann  —  Ber.  37,  4332,  '04.) 
...       (St.  von  Lasczczynski.) 

O  .  0291    (Bodtker  —  Z.  physik.  Chem.  22,  509,  '97.) 


10  •  7  (per  100  g.Sol.)     (de  Coninck— Bull.acad.roy.Belglque,  359, 'oSJ 


G. 

M. 

O 

o-54 

0.028 

18 

0.83 

0.038 

30 

1.03 

0-046 

So 

i  .46 

0.065 

60 

1.86 

0-084 

65 

2.17 

0-098 

Co(I03)2. 


G. 

M. 

G. 

M. 

0.32 

O.OI4 

.  .  . 

o-45 

O.O2O 

1.03 

0.046 

0.52 

O.O23 

0.89 

O.O4O 

0.67 

0.030 

0.85 

0.030 

0.84 

1-02 

per    100   gms. 


0.038 

0.045 

solution. 


o-75 
0.69 


75          

100 

G  =  Gms.    Co(IO3)2 
per  100  Mols.  H2O. 

COBALT    IODIDE    CoI2. 

SOLUBILITY  IN  WATER. 

(Etard  —  Compt.  rend.  113,  699,  '91;  Ann.  chim.  phys.  [7]  2,  537,  '94.) 

The  accuracy  of  these  results  is  doubtful. 

Gms.  CoI2 

t°.       per  100  Gms.  Solid  Phase. 

Solution. 


Co(N03)2. 
SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  439,  'oo.) 


Solid  Phase. 
Co(N03)2.9H20 

Co(NO3)2.6H2O 


Density  of  solution  saturated  at  18°  =  1.575. 


0-033 
0.031 


M  =  Mols.   Co(IO3)a 


—  10 

55-5 

Lol2.± 

0 

58.0 

10 

61.5 

15 

63-2 

20 

65.2 

25 

67 

COBALT    NITRATE    ( 

(Funk  - 

Gms. 

Mols. 

t° 

Co(N03)2 

Co(N03)2 

per  100  Gms. 
Solution. 

per  100 
MoIs.H20. 

-26 

39-45 

6.40 

—  20-5 

42.77 

7-35 

—  21 

41-55 

6.98 

—  10 

43-69 

7.64 

-  4 

44-^5 

7-99 

0 

45-66 

8.26 

+  18 

49-73 

9.71 

Gms.  CoI2 

t°. 

per  100  Gms. 

Solid  Phase. 

Solution. 

25 

67-5      < 

^OlyHjC 

>  (olive) 

30 

7O.O 

" 

40 

75-o        C 

(yellow) 

50 

79.0 

It 

80 

80.0 

« 

no 

81.0 

It 

Gms. 

Mols. 

to      Co(N03)2 
'  per  TOO  Gms. 

Co(N03; 

^    Solid  Phase 

Solution. 

MdJ.nTo. 

41     55-96 

12-5 

Co(N03)2.6H20 

56      62.88 

I6.7 

M 

55    61.74 

I5.8 

Co(N03)2.3H20 

62   62.88 

I6.7 

" 

70    64  .  89 

18.2 

M 

84   68.84 

21.7 

" 

91     77.21 

33-3 

** 

COBALT    NITRATE 


122 


SOLUBILITY  OF  COBALT  NITRATE  IN  GLYCOL. 

(de  Coninck  —  Bull.  acad.  roy.  Belgique,  359,  '05.) 

TOO  grams  saturated  solution  contain  80  gms.  Cobalt  Nitrate. 

COBALT    RUBIDIUM    NITRITE    Rb3Co(NO2)6.H2O. 
100  grams  H2O  dissolve  0.005  gram  of  the  salt. 

(Rosenbladt  —  Ber.  19,  2531,  '86. 

COBALT    SULPHATE    CoSO4.7H2O. 

SOLUBILITY  IN  WATER. 

(Mulder;  Tobler  —  Liebig's  Ann.  95,  193,  '55;  Koppel  —  Wetzel  —  Z.  physik.  Chem.  52,  395,  '05.) 


Gms.  CoSO4 
t  <\                 per  100  Gms. 

Mols.  CoSO4 
per  100                    t  °. 

Gms.  CoSO4              Mols.  CoSO4 
per  100  Gms.                  p^  IOO 

Solution.      Water.           Mols.  ±12U.                                  Solution.       Water.         Mols.  H2O. 

o        20.35     25.55        2.958              35        31.40    45-80        5.31 
5        21.90    28.03        3-251             4o        32-81    48.85        5.664 
10        23.40    30.55        3.540              50        35-56     55-2 

15       24.83    33.05      3.831           60      37.65    60.4 

20        26.58    36.21        4-199              7°        39-66    65.7 
25        28.24    39.37        4.560              80        41.18     70.0 
30        29.70    42.26        4-903            I0°        45-35     83.0 

SOLUBILITY  OF  MIXTURES  OF  CoSO4.7H2O  AND  Na2SO4.ioH2O 
IN  WATER. 

(Koppel;  Wetzel.) 

Gms.  per                             Gms.  per                           Mols.  per 
t».             100  Gms.  Solution.              100  Gms.  H2O.                 100  Mols.  H2O.                Solid  Phase. 

CoS04. 

Na2S04. 

'CoSO4. 

Na2SO4. 

CoSO4. 

Na2S04.' 

O 

5 

16.56 
17.46 

h 

9 

63 
59 

21 
23 

•85 
94 

10.07 

2 
2 

•54 

•77 

I 

I 

•27 
.67 

CoSO4.7H2O  -f 
Na2SO4.ioH2O 

10 

17.90 

ii 

73 

25 

.41 

16.67 

2 

•94 

2 

.11 

.« 

20 

17-59 

16 

43 

26 

65 

24.91 

3 

.09 

3 

.15 

CoNa2(SO4)2.4H2O 

25 

17.06 

15 

7° 

25 

36 

23-32 

2 

•95 

2 

•97 

" 

30 

15-94 

14 

93 

23 

.15 

21  .6l 

2 

•7o 

2 

•74 

" 

35 

15-73 

14 

•52 

22 

54 

20.85 

2 

.62 

2 

.64 

" 

40 

14.87 

14 

22 

2O 

.98 

20.05 

2 

.46 

2 

•53 

" 

18.5 

18.75 

I5 

,61 

28 

.61 

23.82 

3 

•32 

3 

.02 

CoNa2(S04)2.4H2O 

20 

19.30 

15 

10 

29 

.42 

23.01 

3 

.41 

2 

.92 

+  CoS04.7H2O 

25 

20.30 

13 

.60 

30 

•74 

20-58 

3 

•56 

2 

.61 

" 

30 

21.67 

12 

•05 

32 

.70 

18.17 

3 

•79 

2 

•30 

M 

35 

22  .76 

IO 

•43 

34 

.06 

15.61 

3 

•95 

I 

.98 

" 

40 

24.05 

9 

.16 

35 

.01 

I3-72 

4 

.8! 

I 

•74 

" 

18.5 

16.87 

16 

•97 

25 

.50 

2 

.96 

3 

•25 

CoNa2(S04)2.4H20 

20 

15.41 

18 

.12 

23 

.18 

27  .26 

2 

.69 

3 

•45 

+Na2SO4.ioH2O 

25 

10.63 

23 

.26 

16 

•07 

35-17 

I 

.86 

4 

.46 

„ 

30 

6.01 

28 

.67 

9 

.20 

43-74 

I 

.07 

5 

•54 

« 

35 

4-56 

32 

.14 

7 

.19 

50-79 

0 

•835 

6 

•44 

CoNa2(S04)2.4H20 

40 

4-72 

.78 

7 

•45 

50.10 

o 

.864 

6 

•34 

-f-  Na2SO4 

I23 


COBALT    SULPHATE 


SOLUBILITY  OF  COBALT  SULPHATE  IN  METHYL  AND  ETHYL  ALCOHOL 

AND  IN  GLYCOL. 


Solvent. 


Cms.  per  100  Gms. 
Solvent. 


Observer. 


Methyl  Alcohol  (abs.) 


CoSO4.7H2O. 

42  . 8      (de  Bruyn— Z.  physik.  Ch.  10,  784,  '92.) 
50.9 

54-5 

13-3 
1.8 


CoS04. 

3       .«• 
15       ... 

18     1.04 

(93-5%)   3       ••• 
(5o%)       3       ... 
Ethyl  Alcohol  (abs.)  3       ...  2.5 

GIyCQl  •  -(periOOgmS.  (deConinck-Bull.acad. 

solution)  3  .  i          359,  '05.) 
COCAINE    C17H21N04. 
COCAINE    HYDROCHLORIDE    C17H21NO4.HC1. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.;  at  i8°-22°;  Muller  —  Apoth.-Ztg.  18,  248,  '03.) 
Gms.  per  100  Gms.  Solvent. 


roy.Belgique, 


Gms. 


C17H21N04.  Cl7H21N04.HCi: 

per  100  Gms. 
Solvent. 

Water 

25 

0.17 

250 

Ether+H2O 

18-22 

34-o 

Water 

80 

0.38 

IOOO 

H20  +  Ether 

18-22 

0.254 

Alcohol 

25 

20.  o 

38 

Benzene 

1  8-2  2 

100 

Ether  (U.S.P.) 

25 

26.3 

CC14 

J7 

18.5 

Ether 

18-22 

ii.  6 

.  .  . 

Acetic  Ether 

18-22 

58-99 

Chloroform 

18-22 

IOO  + 

Petroleum  Ether  1  8-2  2 

2-37 

CODEINE    C18H21NO3.H2O,  also  the  Phosphate  and  Sulphate. 
COLCHICINE    C22H25NO6. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.;  at  i8°-220,  Muller.) 

Grams,  per  100  Grams  Solvent. 
Solvent. 

Water 

Water 

Water 

Alcohol 

Alcohol 

Ether 

Ether 

Ether  sat.  with  H2O 

H2O  sat.  with  Ether 

Benzene 

Benzene 

Chloroform 

Carbon  Tetra  Chloride  17 

Acetic  Ether 

Petroleum  Ether 


t  °. 

r~ 

Codeine 

Codeine 

~** 

( 

-isH2iNO3  H2O. 

HaPO4.2  Aq. 

H2S04.5  Aq. 

C22H25NO6. 

1  8-2  2 

9.616 

25 

I-I3 

44-9 

3-3 

4-5 

80 

1.70 

217.0 

16.0 

5-o 

25 

62.5 

0-383 

o  096 

60 

108.7 

1.03 

0.27 

25 

8.0 

0.075 

0.64 

18-22 

.  .  . 

0.126 

1  8-2  2 

.  .  . 

.  .  . 

.  .  . 

0.18 

1  8-2  2 

12.05 

18-22 

o-939 

25 

i-iS 

25 

151  .5 

0.015 

100  + 

17 

1.328 

O-I2I 

18-22 

. 

1-342 

1  8-2  2 

0-058 

COLLIDINE  124 

COLLIDINE    (2,  4,  6,  Tri  Methyl  Pyridine)  C6H2N(CH3)3. 

SOLUBILITY  IN  WATER. 

(Rothmund  —  Z.  physik.  Chem.  26,  433,  '98.) 

Gms.  Collidin  per  100  Gms.  0          Gms.  Collidin  per  100  Gms. 

Aq.  Layer.       Collidin  Layer.  Aq.  Layer.     Collidin  Layer. 

5.7  (crit.  t.)  17.20 

10     7.82     41.66       80    1.73    86.12 
20     3.42     54-92       loo    1.78    88.07 

30  2.51  62.80  I2O  1.82  88.98 

40  1.93  70-03  140        2.19        89.10 

60  1.76  80.19  160        2.93        87.2 

180        3.67 
COPPER    ACETATE    Cu(C2H3O2)2.H2O. 

loo  grams  of  glycerine  dissolve  10  grams  of  copper  a.cetate  at  15.5°. 

COPPER    BROMIDE    (ous)    Cu2Br2. 

SOLUBILITY  OF  CUPROUS  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF  POTAS- 
SIUM BROMIDE  AT  i8°-2o°. 

(Bodlander  and  Storbeck  —  Z.  anorg.  Chem.  31,  460,  '02.) 
Millimols  per  Liter.  Grams,  per  Liter. 


KBr. 

Total  Cu. 

Total  Br.    Cu  (ic). 

Cu  (ous). 

KBr. 

Total  Cu. 

Cu  (ic). 

Cu  (ous). 

O 

0.3157 

0.4320  o. 

2096 

0 

.1061 

0 

0.0201 

0 

.0133 

0.0067 

25 

O.II9 

0. 

012 

0 

.107 

2 

.98 

0.0076 

0 

.0007 

O.OO68 

40 

O.2OO 

0. 

013 

0 

.187 

4 

.76 

0.0127 

0 

.0007 

O.OII9 

60 

0.310 

0. 

025 

0 

.285 

7 

0.0197 

0 

.0015 

O.OlSl 

80 

0.423 

0. 

012 

0 

.411 

9 

.53 

0.0266 

0 

.0007 

0.026l 

IOO 

0.584 

...           . 

0 

.584 

ii 

.91 

0.0371 

0.0371 

120 

0.693 

... 

0 

.693 

14 

.29 

O.O44I 

0.0441 

500 

8.719 

... 

8 

.719 

59 

•55 

0.5540 

0.5540 

COPPER    CHLORATE    (ic)    Cu(ClO3)2.4H2O. 
SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  35,  1420,  '02.) 


Gms. 

Mols. 

Gms. 

Mols, 

to         Cu(ClO3)2     Cu(ClO3)2            Solid 
per  loo  Gms.  per  100  Mols.        Phase. 
Solution.          H2O. 

t° 

Cu(ClO3)2    Cu(ClO3)2              Solid 
per  loo  Gms.  per  loo  Mols.          Phase. 
Solution.         H2O. 

—  12 

30-53 

3-43 

Ice 

18 

62.17 

12 

.84 

Cu(C103)2.4H20 

—  31 

54-59 

9-39 

Cu(ClO3)2.4H2O 

45 

66.17 

15 

.28 

" 

—  21 

57-12 

10.41 

" 

59-6 

69.42 

17 

•73 

M 

+  0.8 

58-51 

ii  .02 

" 

76.9 

25 

•57 

.« 

Density  of 

solution 

saturated  at 

18°  = 

1.695. 

COPPER    CHLORIDE    (ic)    CuCl2. 

SOLUBILITY  IN  WATER. 

(Reicher  and  Deventer  —  Z.  physik.  Chem.  5,  560,  '90;  see  also  Etard  —  Ann.  chim.  phys.  [7]  2,  528,  '94.) 

Gms.  CuCl2  Gms.  CuCl2  Gms.  CuCl2 

t°.       per  loo  Gms.  t°.        per  100  Gms.  t°.        per  100  Gms. 

Solution.  Solution.  Solution. 

o    41.4       25    44.0        50    46.65 
10    42.45      30    44-55       60    47-7 

20  43.5  40  45.6  80  49.8 

loo        51.9 
Density  of  solution  saturated  at  o°  =  1.511,  at  17.5°  =  1.579. 


COPPER    CHLORIDE 


SOLUBILITY  OF  CUPRIC  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC ACID  AT  o°. 

(Engel  —  Ann.  chim.  phys.  [6]  17,  351,  '89.) 
Milligram  Mols.  per  10  cc.  Sol.         Sp  Gr.  of  Gms.  per  100  cc.  Sol.          Gms.  per  100  Gms.  Sol. 


fcCuCl2.            HCI.                    Solutions. 

CuCl2. 

HCI. 

CuCl2. 

HCI." 

91 

•75 

o 

•49 

61 

.70 

O-O 

41 

41 

0 

o 

86 

.8 

4 

•5 

•475 

58 

•37 

I  .64 

39 

58 

I 

ii 

83 

.2 

7 

.8 

•458 

55 

•95 

2.84 

38 

37 

I 

95 

79 

•35 

10 

•5 

•435 

53 

•37 

3  -83 

37 

19 

2 

.67 

68 

•4 

20 

•25 

•389 

46 

.01 

7-38 

33 

.11 

5 

•3i 

5° 

•  o 

37 

•5 

•319 

33 

.62 

13  .67 

25 

•5° 

10 

•37 

22 

.8 

70 

•25 

.231 

15 

•33 

25.61 

12 

.46 

20 

.80 

23 

•5 

IO2 

•5 

.288 

IS 

.81 

37  -36 

12 

•27 

29 

.00 

26 

•7 

128 

.0              1.323 

17 

.96 

46.66 

I3 

•57 

35 

.26 

29 

•  o 

Sat.  HCI 

SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC ACID. 

(Engel  —  Ibid,  [6]  17,  372,  '89;  Compt.  rend.  121,  529,  '95.) 


illigram  Mols.  per  10  cc.  Sol.           gD  Qr>  o{           Gn 

is.  per  100  cc.  Sol. 

Gms.  per  100  Gms.  So 

iCu2Cl2. 

HCI.                     Solutions. 

Cu2Cl2. 

HCI: 

CU2C12. 

HCI 

Results  at 

0°. 

o-475 

8 

•975            1-05 

o 

.471 

0 

•327 

O 

.448 

0 

.312 

I  .5 

17 

5 

.049 

I 

.486 

0 

.638 

I 

.418 

0 

.608 

2.9 

26 

o 

.065 

2 

.872 

0 

.948 

2 

.697 

0 

•932 

4-5 

34 

5 

.080 

4 

•457 

I 

•257 

4 

.127 

I 

.164 

8-25 

47 

.8 

•135 

8 

.172 

I 

•743 

7 

.199 

I 

•535 

J5-5 

68 

•5 

.261 

IS 

•7 

2 

•497 

12 

.46 

I 

.980 

33-o 

104 

o 

•345 

32 

.68 

3 

.827 

24 

.30 

2 

•845 

Results  at 

I5°-I< 

)°. 

7-4 

54 

.4                1.19 

7 

•33 

i 

•983 

6 

•159 

I 

.666 

10.8 

68 

.9                1.27 

10 

.69 

2 

•5" 

8 

.422 

I 

•977 

12.8 

75 

.0                1.29 

12 

.68 

2 

•734 

9 

.826 

2 

.119 

16  o 

92.0               1.38 

15 

.84 

3 

•346 

ii 

.48 

2 

.424 

COPPER  CHLORIDE,  AMMONIUM  CHLORIDE  MIXTURES  IN  AQUEOUS 
SOLUTION  AT  30°. 

(Meerburg  —  Z.  anorg.  Chem.  45,  3,  '05.) 


Grams  per  100 
Gms.  Sat.  Solution. 

CuCl2. 
O 
1.9 

3-6 
10.5 

NH4C1. 

29-5 
28.6 

25-9 
I6.5 

19.9 

9.4 

29.4 

4.9 

41.4 

2    I 

43-2 

2  .O 

43-9 

0 

Grams  per  100 
Gms.  Solid  Phase. 


CuCl2. 

6.0 
37-o 
21.7 
28.5 
35-i 
43  i 
5* -9 


NH^Cl. 


48-2 

34-9 
23.1 
18.4 


Solid  Phase 


NH4C1  +  CuCl2  2NH4C1.2H2O 
CuCl2.2NH4C1.2H2O 


13  3 

6  .  6     CuCl2.2NH4C1.2H20  +  CuCl2.2H2O 
CuCl2.2H20 


COPPER    AMMONIUM  126 

CHLORIDE 

COPPER    AMMONIUM    CHLORIDE    CuCl2.2NH4C1.2HaO. 
SOLUBILITY  IN  WATER. 

(Meerburg.) 


Gms. 
«.  e           CuCl2.2NH4Cl                  Solid 
r    '          per  100  Gms.                  Phase, 

Gms. 
to   CuCl2.2NH4Cl                  Solid 
per  100  Gms.                  Phase. 

Solution. 

Solution. 

-10.5 

3-87 

Ice 

30 

27.70 

CuCl2.2NH4Cl. 

2H2O 

-10.8 

20.12 

Ice 

40 

3°-47 

a 

—  II 

20.3 

Ice  +  CuCl2.2NH4C1.2H2O 

5° 

33-24 

u 

—  10 

20.46 

CuCl2.2NH4Cl.2H20 

60 

36.13 

11 

o 

12 

22.02 
24.26 

!! 

£ 

39-35 
43.36 

u 
tt 

20 

25-95 

a 

SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  CUPRIC 
SULPHATE  AT  ABOUT  20°. 

(Bodlander  and  Storbeck  —  Z.  anorg.  Chem.  31,  22,  '02.) 


Millimols  per  Liter. 


Grams  per  Liter. 


CuS04. 

Total  Cu. 

Total  Cl. 

Cu(ic). 

Cu(ous). 

CuS04. 

Total  Cu. 

Total  Cl. 

Cu(ic). 

Cu(ous). 

0 

2. 

880 

5-312 

2.258 

0. 

622 

0.0 

0.183 

0.188 

0-143 

0.040 

0.987 

3- 

602 

4.908 

3  -145 

O, 

•457 

0.158 

o.  229 

0.174 

O.  2OO 

0.029 

i-975 

4- 

553 

4.687 

4.131 

0, 

,422 

0.315 

0.290 

0.166 

0.263 

0.027 

2.962 

5- 

193 

4.256 

4.625 

o. 

509 

0-473 

0.330 

0.151 

0.292 

0.032 

4-937 

7- 

276 

4.329 

6.546 

0. 

73° 

0.788 

0.463 

o.i54 

0.4l6 

0.046 

SOLUBILITY  OF  CUPROUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  POTASSIUM 
CHLORIDE  AT  i8°-2o°  EXCEPT  DETERMINATIONS  IN  3RD,  7™,  STH,  AND 

LAST   LINE,    WHICH  ARE  AT    1 6°. 

(Bodlander  and  Storbeck.) 


Millimols  per  Liter. 


Grams  per  Liter. 


KC1. 

Total  Cu. 

Total  Cl. 

Cu(ic). 

Cu(ous). 

kci. 

Total  Cu. 

Total  Cl. 

Cu(ic), 

Cu(ous) 

0 

2.851 

5-436 

2.222 

0.629 

o.o 

O. 

181 

0.193 

0. 

141 

0.040 

2.5    i-955 

6.015 

I.42I 

0-534 

0.186 

0. 

124 

0.213 

0. 

090 

0.034 

5 

1.522 

7.525 

I.  008 

0.514 

0.373 

0. 

097 

0.267 

o. 

069 

0.033 

10 

1.236 

11-735 

0-475 

0.761 

0.746 

0. 

079 

0.416 

0. 

030 

0.048 

20 

1.446 

21.356 

0.324 

I.  122 

1.492 

o. 

092 

0-759 

o. 

02  1 

0.071 

5° 

2.411 

not  det. 

0.1088     2.302 

3.730 

0. 

J53 

not  det. 

0. 

007 

o.  146 

100 

4.702 

a 

o.ooo 

4.702 

7.460 

o. 

299 

« 

o. 

000 

0.299 

2OO 

9.485 

tt 

0.000 

9.485 

14.920 

0. 

603 

(I 

0. 

opo 

0.603 

1000 

97-o 

n 

o.ooo 

97.0 

74.60 

6. 

170 

(4 

o. 

000 

6.170 

2OOO 

384.0 

n 

0.000 

384.0 

149.2 

24. 

42 

(1 

0. 

000 

24.420 

SOLUBILITY  OF  COPPER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

CHLORIDE. 

(Hunt  —  Am.  J.  Sci.  [2]  49,  154,  '70.) 

Grams  CuCl2  per  100  cc.  Solution  of: 


II 
40 
90 


Sat.  NaCl. 

8-9 
11.9 
16. 9 


15%  NaCl.  5%  NaCl. 

3-6 

6.0  i.i 

10.3  2.6 


127  COPPER    CHLORIDE 

SOLUBILITY  OF  COPPER  CHLORIDE  AND  POTASSIUM  CHLORIDE  DOUBLE 

SALTS  AND  MIXTURES  IN  WATER. 

(Meyerhoffer  —  Z.  physik.  Chem.  5,  102,  '90.) 

Cl  per  i  Gram  Solution.  Mols.per  iooMols.H2O. 

*°-          'Present  as      Present  as'  r  r.                                                     JjJJ 

CuCl2.              KC1.  CuCl2'          KCL 

39.4            0.120         0.107  5.56            9.93       CuCl2.2KCl.2H20  +  KC1 

49.9            0.129         O.II5  6.39         II-4 

60.4  O.I42         O.I25  7.71          I3-6 

79.1         0.168      0.142  ii. i         18.8 

90.5  0.188      0.154  14.9        24.4 

93-7            0.194         0-156  l6.2            26.0         CuCl2.KCl  +  KCl 

98.8  0.197         O.l62  17.5            28.7 

O                0.214        O.O2I  9-84           1-94      CuCl2.2KC1.2H2O  +  CuCl2.aH2O 

39.6  0.232       0.049  I2-9          5-44 

50.1  0.233       0.059  13.7          6.90 

52.9  0-241       0.062  14.8           7.63 

60.2  0.246         0.066  15.8               8.49       CuCl2.KCl  +  CuCI2.2H20 

72.6        0.255       0.063  16.8          8.35 

64 . 2                                      ...  14.9            1 1  . 6         CuCl2.2KC1.2H20  -f  CuCl2.KCl 

72.5               ...                ...  14.8            15.0         CuCl2.KCl 


SOLUBILITY  OF  CUPRIC  CHLORIDE  IN  SEVERAL  SOLVENTS. 

(Etard  —  Ann.  chim.  phys. [7]  2,  564,  '94;  de  Bruyn  —  Z.  physik.  Chem.  10,  783,  '92;  de  Coninck  — 
Compt.rend.  131,  59,  'oo;  St.  von  Laszczynski  —  Ber.  27,  2285,  '94.) 

Grams  CuCl2  per  100  Grams  Sat.  Solution  at: 


ouiveiu. 

Methyl  Alcohol 
Ethyl  Alcohol 

0°. 

36 

32 

15°. 

40.5  (deB.) 
35.0  (deB.) 

20°. 
36.5 

35-7 

4o°.         80°. 
37.0       ... 
39.0 

Propyl  Alcohol 

29 

30 

•5 

30 

•5 

Iso  Propyl  Alcohol 

.  .  . 

16 

.0     30 

.0 

n  Butyl  Alcohol 

15 

15 

•3 

16 

.0     16 

•5 

Allyl  Alcohol 

23 

.  .  . 

23 

-0 

Ethyl  Formate 

IO 

.  .  . 

9 

.0 

8 

•  o 

Ethyl  Acetate 

.  .  . 

O 

.0 

2 

•5       i 

•3  (72°) 

Acetone  (abs.) 

8.86* 

8.92f 

2 

.88 

(18°)     .. 

i 

•40  (56°; 

Acetone  (80%) 

18 

9* 

. 

Ether 

0.043  (II0) 

o. 

ii 

. 

*  (CuCl2.2 

Aq.) 

t  (CuCl2.2  Aq.) 

$  (23°  CuCl2.2  Aq.) 

For  the  solubility  of  cupric  chloride  in  mixtures  of  a  number  of 
organic  solvents,  see  de  Coninck. 


COPPER    CHLORIDE 


128 


IN  AQUEOUS  ALCOHOL  AT  11.5°. 

Chem.  22,  507,  '97.) 

indicated  amounts  of  CuCl2  were 
The  solutions  shaken  two  hours, 


SOLUBILITY  OF  CUPRIC  CHLORIDE 

(Bodtker  —  Z.  physik. 

10  gms.  of  CuCl22H2O  and  the 
added  to  20  cc.  portions  of  alcohol. 
5  cc.  portions  withdrawn. 

Vol.  %    Gms.  CuCl2    Gms.  per  5  cc.  Solution. 
Alcohol.      Added.          H2O.  CuCl2.' 

89.3  o.o  0.794  1.137 

92.0  o.o  0.648  1.090 

96.3  o.o  0.478  1.116 

99.3  o.o  0.369  i. 208 


COPPER    NITRATE    (ic)  Cu(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt,  3,  440,  'oo.) 


Vol.  %       Gms.  CuCl2 

Gms.  per  5  cc.  Solution. 

Alcohol.        Added. 

H2O.              CuCl2. 

99-3         0.223 

0.330            1.295 

99.3         0.887 

0.247            1.639 

99.3         1-540 

O.I9I            2.o86 

99-3       i-957 

0.164            2.400 

Gms. 

Mols. 

t°. 

Cu(N03)2 
per  100  Gms. 

Cu(N03)2 
per  100 

Solid  Phase. 

Solution. 

Mols.  H20 

, 

-23 

36.08 

5-42 

Cu(NO3)2.9H20 

—  20 

40.92 

6.65 

" 

—  21 

39-52 

6.27 

Cu(NO3)2.6H2O 

O 

45-00 

7.87 

" 

+  10 

48.79 

9-T5 

" 

18 

53-86 

ii  .20 

u 

20 
26.4 

25 
40 

60 

86 

ii4-5 


Gms.  Mols. 

Cu(N03)2      Cu(N03)2 
per  100  Gms.     per  100        Solid  Phase. 
Solution.       Mols.  H2O. 

55.58    I2.O   Cu(NO3)2.6H2O 
I6.7 
14.4 

15-2 
17.2 
20.0 


63-39 

60. 01 
61 .51 
64.17 

67-51 
77-59 


Cu(N03)2.3H20 


33-3 


Density  of  solution  saturated  at  18°  =  1.681. 


COPPER    SULPHATE    CuSO4.5H2O. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  528,  '94;  Patrick  and  Aubert  —  Trans.  Kansas  Acad.  Sci.  19,  '74  ;  at 
—  Z.  E!ec 


[5°,  Cohen 


lectrochem.  9,  433,  '03;  at  25°,  Trevor  —  Z.  physik.  Chem.  7,  470,  '91.) 
Gms.  CuSO4  per  100  Gms. 


1    . 

O 
10 

Solution. 
12-5 
14.8 

Water.' 
14-3 
17.4 

20 

25 

17.2 
I8.S 

20-7 
22-7 

30 

40 

20.  o 

22.5 

25.0 
28.5 

50 

25.0 

33-3 

i  . 

Solution. 

Water.  " 

60 

28-5 

40.0 

80 

35-5 

55-o 

100 

43-o 

75-4 

120 

44-o 

78.6 

I4O 

44-5 

80.2 

1  60 

44-o 

78.6 

180 

43-o 

75-4 

SOLUBILITY  OP  COPPER  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  SUL- 
PHURIC ACID  AT  o°. 

(Engel  —  Compt.  rend.  104,  507,  '87.) 

Milligram  Equiv,  per  10 
Gms.  H2O. 


H2S04. 

CuSO4. 

o.o 

18.6 

4.14 

17.9 

14.6 

19.6 

31.0 

12.4 

54-2 

8.06 

56-25 

7-75 

71.8 

5-o 

Sp.  Gr.  of 
Solutions. 

I.I44 

Grams  per  TOO  Grams 
H20. 

H2S04. 

o.oo 

CuSO4. 
14.85 

I  -143 
I.I58 

2.03 
7.l6 

14.29 

J5-65 

I  .170 

I-I95 
I  .211 

15.20 
26.57 

27-57 

9.90 

6-43 
6.19 

1.224 

35-2 

3-99 

i29  COPPER    SULPHATE 

SOLUBILITY  OF  COPPER  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  AMMO- 
NIUM SULPHATE  AT  o°. 

(Engel  —  Com pt.  rend.  102,  114,  '86.) 


Milligram  Equiv.  per 
10  cc.  Solution. 

Sp.  Gr.  of 
o  utions. 

Grams  per 
loo  cc.  Solution. 

(NH4)2S04. 

CuSO4. 

(NH4)2S04. 

CuS04. 

o.o 

18.52 

I.I44 

0.0 

14.79 

5-45 

20.15 

I  .190 

3.6l 

16.09 

7-o 

10-5 

I.IOS 

4-63 

8.38 

7-4 

9-1 

1.099 

4.90 

7.26 

8.45 

6.425 

1.0815 

5-59 

5-13 

II  .35 

3-7 

I  .071 

7  -51 

2  95 

18.6 

1.178 

1.082 

12.31 

o-94 

31.2 

i  .0 

I  .Il6 

20.65 

0.80 

MIXTURES  OF  COPPER  AMMONIUM  SULPHATE  AND  NICKEL  AMMONIUM 
SULPHATE  IN  WATER  AT  i3°-i4°. 

(Fock  —  Z.  Kryst.  Min.  28,  394,  '97.) 

CuSO4.(NH4)2SO4.6H2O  —  NiSO4.(NH4)2SO4.6H2O. 

Mol.  %  in  Solution.  Mols.  per  100  Mols.  H2O.          Mol.  %  in  Solid  Phase. 


Cu. 

Salt. 

Ni  Salt. 

Cu  Salt. 

Ni  Salt.  ' 

Cu. 

Salt. 

Ni  Salt." 

O 

•  OO 

IOO 

.00 

0 

.00 

0.521 

0 

•  OO 

IOO 

.00 

33 

•34 

66 

.66 

0 

.1476 

O 

•295 

10 

.29 

89 

•71 

43 

•95 

O 

.2664 

0 

.2089 

30 

•59 

69 

.41 

73 

^89 

26 

.20 

0 

.4165 

0 

.1449 

52 

•23 

47 

•77 

79 

.92 

20-08 

O 

•4785 

0 

.1202 

78 

.80 

21 

.20 

IOO 

.00 

o 

.00 

I 

•0350 

o 

•  OO 

IOO 

.0 

0 

.00 

MIXTURES   OF  COPPER  AMMONIUM   SULPHATE   AND  ZINC  AMMONIUM 
SULPHATE  IN  WATER  AT  13°— 14°. 

(Fock.) 

CuSO4.(NH4)2SO4.6H2O  —  ZnSO4.(NH4)2SO4.6H2O. 

Mol.  %  in  Solution.  Mols.  per  100  Mols.  H2O.  Mol.  %  in  Solid  Phase. 


Cu.  Salt. 

Zn  Salt. 

Cu  Salt.. 

Zn  Salt. 

Cu.  Salt. 

Zn  Salt. 

4-97 

95-03 

O.O422 

o  .  8069 

2-39 

97.6l 

10.65 

89-35 

o  •  0666 

0-5638 

4-52 

95-48 

19.24 

80.76 

0.1218 

O.S"5 

9-03 

90.97 

30.19 

69.81 

0.2130 

0.4924 

14.67 

85-33 

44.44 

55-56 

0.3216 

O.4O22 

22  .62 

77-38 

100.00 

o.oo 

1-035 

O-OOO 

IOO 

0-000 

SOLUBILITY   OF   COPPER   SULPHATE   IN   AQUEOUS   SOLUTIONS   OF 
MAGNESIUM  SULPHATE  AT  o°. 

(Diacon  —  Jahresber.  Chem.  61,  '66.) 

Grams  per  TOO  Gms.H2O.  Solid  Grams  per  100  Gms.  H2O.  Solid 

CuS04.     "MgS04.   '  CuSCv      MgS04. 

O  26.37  MgSO4.6H2O  12.03      I5    67 

2.64     25.91  *3-6i       8.64 

4-75     25.30  "  14-99      o.oo 

9-01      23  . 30         MgSO4.6H2O  +  CuSCVsHzO 


COPPER    SULPHATE 


130 


COPPER  SULPHATE,  MANGANESE  SULPHATE,  MIXED  CRYSTALS  AT  25' 

(Stortenbecker  —  Z.  physik.  Chem.  34,  112,  *oo.) 
Mols.  per  100  Mols.  H2O. 


Gms.  per  ioq  Gms.  H2O. 
CuSO4.  MnSO4. 

Triclinic  Crystals  with  sH2O. 

20-2  O 

19.76  3.69 


13.65  3I-52 

ii. 61  39.41 

9-39  46.77 

6-47  53-39 

3-oJ  58-93 

o.o  61.83 

Monoclinic  Crystals  with  ?H2O. 


Mol.  %  Cu         Mol.  %  Cu 


Cu. 

Mn.   ' 

in  Solution. 

in  Crystal: 

2.282 

O 

100 

100 

90-5 

99-3 

2.23 

0-44 

83.5 

74-1 

97-3 

57-7 

95  -1 

31.0 

81.3 

i-54 

3  -76 

29.0 

26.1 

70.4 

i  .31 

4.70 

21.8 

21  .2 

42  .6 

20.0 

34-4 

i.  06 

5-59 

15-9 

22  .9 

13-45* 

I5.2* 

o-73 

6-37 

10.27 

10-5 

5-o 

4-9 

0-34 

7-03 

4.6 

2.31 

2.15 

o.o 

7-375 

o.o 

100.  0 

9-39 
6.47 
o.o 


46.77 
53-39 


i  .06 

o-73 
o.o 


5-58 
6.37 

8±* 


20-0 
IS-9 

!3-45 

10.27 

4.6* 

o.o 


28.2 
23-5 

20.8 

16.0 

5.8* 

100 


*  Indicates  points  of  labil  equilibrium. 


COPPER    SULPHATE,    ZINC    SULPHATE,  MIXED    CRYSTALS    IN    WATER. 

(Stortenbecker  —  Z.  physik.  Chem.  22,  62,  '97.) 


Triclinic  Crystals  with  sH2O. 


Monoclinic  Crystals  with  7H2O. 


Rhombic  Crystals  with  7H2O. 


ols.  per  too 

Mols.  H2O. 

Mol.  %  Cu 

Mol.  %  Cu 

Cu. 

Zn. 

in  Solution. 

in  Crystals. 

2.28 

O 

100 

100 

1.83 

2-o8 

46.8 

94-9 

I.4I 

3-60 

28.1 

86.4 

I.I9 

5-01 

19.2 

77-9 

1.86 

3-36 

36.2 

40.4 

1.22 

4-45 

21-5 

29-5-31-9 

1.  01 

4-72 

17.6 

24  .  1-28  . 

0.82 

5-03 

14.0 

19.0-22. 

0.51 

5-59 

8.36 

12.4-14.9 

0.30 

5-56 

4.87 

7.02 

o.o 

6.42 

o.o 

0 

1.19 

5.01 

19-2 

5.01 

0.51 

5-59 

8.36 

1.97 

0.267 

5-77 

4.42 

*•?$ 

o.o 

5-94 

o.o 

0-00 

131  COPPER    SULPHATE 

SOLUBILITY  OF  COPPER  SULPHATE,  SODIUM  SULPHATE  MIXTURES  IN 

WATER. 

(Koppel  — Z.  physik.  Chem.  42,  8,  'oi-'o2;  Massol  and  Maldes  —  Compt.  rend.  133,  287,  '01.) 


O 
10 

15 
17.7 

23.0 

40.15 
17.7 

23 
40.15 

18 

20 

25 
30 

33-9 

37-2 
30 
30.1 
30 


Gms.  per  100  Gms. 
Solution. 

CuSO4. 

Na2S04. 

13.40 

6.23 

14-90 

9.46 

I5.I8 

11.64 

14-34 

I3-34 

14.36 

12  .76 

J3-73 

12.26 

14.99 

13.48 

16.41 

II  .35 

20.56 

8.0 

13-53 

13.84 

u-34 

15  .70 

6.28 

21  .20 

2  .607 

28.38 

J-475 

32-30 

1.494 

31.96 

5-38 

22.17 

3-69 

25-37 

J-57 

32.09 

Mols.  per  100  Mols. 

Na2SO4.' 
0.98 
I.56 
2.02 

2-34 
2.21 
2.10 

2-39 

1.99 
1.47 
2.41 

2-73 

3-70 

5-21 

6.18 
6.08 


CuSO4 

1.88 
2.23 
2.23 
2.24 
2.23 

2.10 

2-37 
2-57 
3-25 

2  .IO 
I.76 
0.98 

o-43 
0.25 
0.25 


Solid  Phase. 
CuS04.5H20  +  Na2S04.ioH20 


CuS04.Na2S04.6H2O 


CuS04.Na2S04.6H20  +  CuSO4.5H2O 


CuSO4.Na2SO4.6H2O  +  Na2SO4.ioH2O 


} 


CuSO4.Na2SO4.6H2O  +  increasing 
amts.  of  Na2SO4.ioH2O 


SOLUBILITY    OF   COPPER   POTASSIUM   SULPHATE    CuK2(SO4)2.6H2O   in 

WATER  AT  25°. 
100  gms.  H2O  dissolve  11.14  gms.  CuK2(SO4)2. 

(Trevor  —  Z.  physik.  Chem.  7,  470,  '91. 

SOLUBILITY  OF  COPPER  SULPHATE  IN  METHYL  AND  ETHYL  ALCOHOL, 

ETC. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  786,  '92;  de  Coninck  —  Bull.  acad.  roy.  Belgique,  257,  '05.) 


Solvent. 

Methyl  Alcohol  Abs. 

93-5% 
50% 
Abs. 

Ethyl  Alcohol  Abs. 

Glycol 

Glycerine 


Gms.  per  100  Gms.  Solvent.   SOLUBILITY    IN   AQUEOUS 


Gms.  CuSO4.5H2O 
per  100  g.  Solvent. 

15-3 

3-2 

0.25 


CuSO4. 

CuS04.5H20. 

ALCOI 

18       1.05 

I5.6 

(Schiff  —  Liebij 

18 
18 

o-93 
0.40 

Wt.% 
Alcohol. 

3 

13-4 

10 

3 

i  .1 

20 

14.6 

7.6* 

40 

15  .5 

3°-o 

*  Per  100  g.  sol. 


COPPER    SULPHIDE    CuS. 

SOLUBILITY  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Stolle  —  Z.  Ver.  Zuckerind.  50,  340,  *oo.) 

Gms.  CuS  per  Liter  of  Aq.  Sugar  Solution  at: 


%  Sugar 
in  Solvent. 

10 
30 
50 


0.5672 
0-8632 
0-9076 


45°- 

0.3659 
0.7220 
1.0589 


75°. 

I-I345 
1.2033 
I . 2809 


COPPER    TARTRATE  132 

COPPER    TARTRATE    CuC4O6H4.3H2O. 


SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder  —  Bull.  soc.  chim.  [3]  33,  751,  '05.) 


Gms. 

Gms. 

Gms. 

t  ° 

CuC4OeH4.3H2O 

t°     ' 

:uC406H4.3H2O 

t  •. 

CuC406H4.3H20 

* 

per  100  cc. 

per  100  cc. 

per  100  cc. 

Solution. 

Solution. 

Solution. 

15 

0.0197 

40 

O.I42O 

65 

0.1767 

20 

0.0420 

45 

0.1708 

70 

0.1640 

25 

o  .  0690 

50 

0.1920 

75 

0.1566 

30 

o  .  0890 

55 

0.2124 

80 

0.1440 

35 

0.1205 

60 

0.1970 

85 

0.1370 

CRESOL    C6H4(OH).CH3    o,  m  and  p. 

SOLUBILITY  IN  WATER  AT  20°. 

(Vaubel  —  J.  pr.  Chem.  [2]  52,  72,  '95.) 

TOO  grams  of  the  saturated  aqueous  solution  contain  : 
f. A. 

2.45  grams  o  cresol,     2.18  grams  m  cresol,      1.94  grams  p  cresol. 
DISTRIBUTION  OF  CRESOL  BETWEEN  WATER  AND  ETHER, 

(Vaubel  — J.  pr.  Chem.  [2]  67,  472,  '03.) 
Composition  of  Solvent.  Gms.  Cresol  in  H^O  Layer.      In  Ether  Layer. 

200  cc.  H2O+ioo  cc.  Ether  0-0570  i  .0760 

200  cc.  H2O  +  2oo  c.c.  Ether  0.0190  i  -1144 

CUMINIC    ACID   C3H7C6H4.COOH   (p  Iso  Propyl  Benzoic  Acid). 
SOLUBILITY  IN  WATER  AT  25°. 

(Paul  —  Z.  physik.  Chem.  14,  in,  '94.) 

1000  cc.  sat.  solution  contain  0.1519  gm.  or  0.926  millimol  Cuminic 
Acid. 

PseudoCUMIDINE  (CH3)3.C6H2.NH2  (sym.   5  Amino,  i,  2,  4,  Trimethyl 
benzene). 

SOLUBILITY  IN  WATER. 

(Ljwenh.-rz  —  Z.  physik.  Ch.  25,  412,  '98.) 

| 

t°.  19-4°.  23.7°.  28.7°. 

Gms.  $  Cumidine  per  liter  H,O        i .  198         i .  330         i  .498 


CYANOGEN    CN. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  20°. 

(Gay  Lussac.) 

Solvent.  Vols.  CN  per  i  Vol.  Solvent. 

Water  4.5 

Alcohol  23  .o 

Ether  5  .o 

Oil  of  Turpentine  5.0 


133  DIDYMIUM    SULPHATE 

DIDYMIUM    SULPHATE    Di2(SO4)3. 

SOLUBILITY  IN  WATER. 

(Marigr  ac  —  Ann.  chim.  phys.  [3]  38,  170,  '53.) 

Gms.Di2(SO4)3  Solid  Gms.Di2(SO4)3 

t°.  per  ioo  pT;1"  t°.  per  ioo 

Gms.H-jO.  Gms.HzO.  Phase- 

12  43.1  Di2(S04)3              ?  34.0  Di,(S04)3.6H20 

18  25.8  19  n.7  Di2(S04)3.8H20 

25  20.6  40  8.8                     " 

38  13.0  50  6.5 

50  ii. o  ioo  1.8                     " 


DIDYMIUM    POTASSIUM    SULPHATE    K2SO4.Di2(SO4)3.2H2O. 

(Marignac.) 

ioo  gins.  H2O  dissolve  1.6  grains  double  salt  at  18°. 


ERBIUM    SULPHATE    Er2(SO4)3. 

SOLUBILITY  IN  WATER. 

(Hoglund.) 

ioo  gms.  H2O  dissolve  43.0  gms.  Er2(SO4)3  at  o°. 

ioo  gms.  H2O  dissolve  23.0  gms.  Er2(SO4)3.8H2O  at  20°. 

ERYTHRITE  CH2OH(CHOH)2CH2OH. 

ioo  grams  saturated  solution  in  pyridine  contain  250  gms.  at  26°. 

(Holty  — J.  Physic.  Chem.  9,  764,  \>5.J 

ETHANE    C2H8. 

SOLUBILITY  IN  WATER. 

(Winkler  —  Ber.  34,  1421,  '01.) 
t°.  /9.  /3'.  q.  t°.  ft.  0'.  q. 

o  0.0987  0.0982  0.0132  40  0.0292  o  0271  0.0037 

5  0.0803  0.0796  0.0107  50  0.0246  0.0216  0.0029 

10  0.0656  0.0648  0.0087  60  0.0218  0.0175  0.0024 

J5  °-°55°  0.0541  0.0073  7°  0-0195  0-0135  0.0018 

20  0.0472  0.0462  0.0062  80  0.0183  0.0097  0.0013 

25  0.0410  0.0398  0.0054  90  0.0176  0.0054  0.0007 

30  0.0362  0.0347  0.0049  Io°  0.0172  o.oooo  o.oooo 

ft  =  Absorption  coefficient,  i.e.,  the  volume  of  gas  (reduced  to  o° 
and  760  mm.)  absorbed  by  i  volume  of  the  liquid  when  the  pressure 
of  the  gas  itself  without  the  tension  of  the  liquid  amounts  to  760  mm. 

/?'  =  Solubility,  i.e.,  the  volume  of  gas  (reduced  to  o°  and  760  mm.) 
which  is  absorbed  by  one  volume  of  the  liquid  when  the  barometer 
indicates  760  mm.  pressure. 

q  =  the  weight  of  gas  in  grams  which  is  taken  up  by  TOO  grams  of 
the  pure  solvent  at  the  indicated  temperature  and  a  total  pressure 
(that  is,  the  partial  pressure  of  the  gas  plus  the  vapor  pressure  of  the 
liquid  at  the  absorption  temperature)  of  760  mm. 


ETHER 


134 


ETHER    (C2H6)2O. 

RECIPROCAL  SOLUBILITY  OF  ETHER 


AND  WATER. 


(Klobbie  — Z.physik.Chem.  24,  619,  '97;  Schuncke  —  Ibid.  14,  334,  '94;  St.Tolloczko  —  Ibid. 20,  407, 

'96.) 


Solubility  of  Ether  in  Water. 
Lower  Layer  —  Aqueous. 

,      Gms.  (C2H5)2O  per  100  Cms. 


Solubility  of  Water  in  Ether. 
Upper  Layer  —  Ethereal. 

Gms.  H2O  per  100  Gms. 


Water. 

Solution. 

o 

13.12 

ii.  6 

5 

II-4 

10.2 

10 

9-5 

8.7 

15 

8.2 

7.6 

20 

6  -95 

6-5 

25 

6.05 

5-7 

30 

5-4 

5  -1 

*4o 

4-7 

4-5 

*5o 

4-3 

4.1 

*6o 

3-8 

3-7 

*7o 

3-3 

3-2 

*8o 

2.9 

2.8 

Ether. 
I  .01 

Solution 
I  .0 

1.  06 

1.05 

1.  12 

I  .12 

(2.6,8.) 

.16 

1  -r5 

.20 

1.20 

(2.65,8.) 

.26 

1.26 

•33 

1.32 

•52 

1-50 

•73 

I  .7 

1.83 

1.8 

2  .04 

2  -O 

2.25 

2  .2 

*  Indicates  determinations  made  by  Synthetic  Method,  for  which  see  page  9. 

ioo  cc.  H2O  dissolve  8.11  cc.  ether  at  22°;  Vol.  of  solution  107.145  cc., 
Sp.  Gr.  0.9853. 

ioo  cc.  ether  dissolve  2.93  cc.  H2O  at  22°;  Vol.  of  solution  103.282, 

Sp.  Gr.  0.7164.  (Herz  — Ber.  31,  2671,  '98.) 

For  recent  determinations  of  the  density  of  ether,  see  Christomanos  — 
Z.  anorg.  Chem.  45,  136,  '05. 

SOLUBILITY  OF  ETHER  IN   AQUEOUS    SOLUTIONS    OF    HYDROCHLORIC 

ACID. 

(Schuncke  —  Z.  physik.  Chem.  14,  334,  '94;  in  38.52%  HC1,  Draper  —  Chem.  News,  35,  87,  '77.) 


In38.52%HCl. 


In  3i.6i%HCl. 


HC1. 


cc.  Ether 

cc. 

Ether              Gms.  per  i  Gram  H2O. 

cc.  Ether    Gms.  per 

i  g.  H20. 

t°. 

per  ioo  cc. 
Solvent. 

per  ioo  cc. 
Solvent.                      HC1. 

(C2Hs)2O.          Solvent. 

'     HCl. 

(C2H6)20. 

-6 

181 

149 

0.4622 

I 

•387 

67.2 

0 

•253 

0.5637 

o 

177 

•5 

142 

0.4622 

I 

58.3 

0 

o  .  4863 

+  6 

172 

•5 

I3I 

5 

0.4622 

I 

.2075 

5I-I 

0 

253 

0.4231 

i5 

163 

121 

7(i4°) 

0.4622 

I 

•Io75 

40-5 

o 

•253 

0.3299 

20 

158 

116 

.9(20.8°) 

0.4622 

I 

.0005 

33-i 

0 

•253 

0.2688 

26 

J35 

104. 

2 

0.4622 

0 

.9360 

27-5 

0 

•253 

O-222I 

In  i2.58%HCl. 


In  3.65  %  HC1. 


AO              cc.  Ether  per 

Gms.  per  i  Gram  H2O. 

cc.  Ether  per 

Gms.  per  i  Gram  H2O. 

ioo  cc.  Solvent. 

HCl. 

(C2H5)20. 

ioo  cc.  Solvent. 

HCl. 

(C2H5)20. 

-6 

26 

•45 

O 

.144 

0 

.2106 

19 

•23 

0-0308 

0 

1454 

0 

22 

.19 

O 

.144 

0 

.1748 

4-6 

19 

.18 

O 

.144 

0 

•!503 

14 

•3i 

0.0308 

O 

.1070 

15 

IS 

.61 

O 

.144 

0 

.I2IO 

II 

•83 

0-0308 

O 

.0868 

20 

13 

•76 

0 

.144 

O 

.1059 

10 

•52 

0-0308 

O 

.0769 

26 

12 

.70 

O 

.144 

o 

.0970 

9 

.24 

0-0308 

0 

.0673 

i35  ETHEK 

SOLUBILITY  OF  ETHER  IN  AQUEOUS  SALT,  ETC.,  SOLUTIONS  AT  18°. 

(Euler  — Z.  physik.  Chem.  49,  306,  '04.) 


Aq.  Solu- 
tion of: 

Gms.  per 
Liter  Added 
Salt. 

Gms.  (C2HC)20 
per  TOO  cc. 
Solvent. 

Aq.  Solu- 
tion of: 

Gms.  per 
Liter  Added 
Salt. 

Gms.  (C2H 
per  TOO  c 
Solvent. 

Water 

0-0 

7-8 

Na2S04 

59-54 

3-7 

KNO3 

ioi  .19 

5-4 

Mannite 

91.06 

6.7 

KC1 

73-6 

4-7 

H2S04 

49.0 

6.6 

Lid 

42.48 

5-2 

u 

122.5 

5-65 

NaCl 

58-5 

4-5 

11 

245.0 

4-55 

SOLUBILITY  OF  ETHER  IN  AQUEOUS  ETHYL  ALCOHOL  AND  IN  AQUEOUS 
METHYL  ALCOHOL  MIXTURES  AT  20°. 

(Bancroft  —  Phys.  Rev.  3,  122,  *95-'96.) 

In  Ethyl  Alcohol.  In  Methyl  Alcohol. 

Per  5  cc.  Alcohol.  Per  5  cc.  Alcohol.  Per  i  cc.  CH3OH.  Per  i  cc  CH3OH. 


cc.H20 

.*  cc.(C2H5)2O.t  cc.H2O.*  cc.(C2H5)2O.t 

cc.H2O. 

cc.(C2H5)2O.  cc.H2O. 

cc.(C2H5-)20: 

50 

1.30        4.45          7-o 

10 

I.I3            0.83 

1.  80 

25 

1.70            4-0                 7.8 

7 

0-85            0.64 

3-00 

IO 

2.41        3.87          8.0 

4 

O-6o           0.52 

5-o 

8 

3.35        3.10         10.  o 

2-5 

0.56           O-44 

IO-O 

6 

5.10        2.08         15.0 

1.8 

0.63            0.45 

15.0 

5- 

21     6.00         1.77         17.5 

I  .0 

1.23 

*  Saturated  with  ether. 

t 

Saturated  with  water. 

ETHYL    ACETATE    CH3COOC2H6. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SALT  SOLUTIONS  AT  28°. 

(Euler  —  Z.  physik.  Chem.  31,  365,  '99;  49,  306,  '04.) 


Cone,  of  Salt 
Solution. 

CH3COOC2Hs 

per  Liter. 

Solvent             f 

Cone,  of  Salt 
Solution. 

CH3COOC2H6 
per  Liter. 

Solvent. 

Nor-   Gms   per 
mality.    Liter. 

Gram 
Mols. 

Grams. 

Nor-  Gms.  per    Gram 
mality.     Liter.       Mols. 

Grams. 

Water 

0 

0 

0.825 

75- 

02 

NaCl(at  18°) 

\      14.62 

0. 

76 

67.0 

KN03 

£ 

50-59 

0.77 

67. 

81 

«           it 

i      29.25 

0. 

67 

59- 

0 

a 

I 

ioi.  19 

0.72 

63- 

40 

(t           it 

I      58.5 

O. 

51 

45- 

o 

it 

2 

202.38 

0.625 

55- 

04 

Na2S04 

I       71.08 

0. 

465 

40. 

96 

KC1 

\ 

18.4 

0.747 

65- 

79 

"      (at  18°) 

i     35-54 

O. 

61 

54- 

0 

it 

\ 

36.8 

0.685 

65- 

33 

tt          ti 

i     71.08 

O. 

42 

37- 

0 

it 

I 

73-6 

0-575 

50- 

64 

MgS04 

J     16.30 

O. 

733 

64. 

55 

t( 

2 

147.2 

0.41 

36. 

ii 

tt 

i     32-6 

o. 

655 

57- 

68 

NaCl 

I 

14.62 

0-745 

65- 

61 

tt 

i     65.21 

0-505 

44. 

47 

« 

29.25 

0.677 

59.62 

ZnSO4 

\       20.  l8 

o. 

733 

64- 

55 

ti 

I 

58.5 

0-545 

47- 

99 

«  . 

i    40.36 

0. 

653 

57- 

5° 

« 

2 

117.0 

0.315 

27. 

74 

" 

i    80.73 

0. 

500 

44. 

03 

In  Methyl  Alcohol. 

In 

Acetone. 

Per  i  cc.  CH3OH. 

Per  i 

cc.  (CH3)2CO. 

cc.  HzO.      CHaCOOCzHs. 

cc.  H2O. 

CH3COOC2H8. 

10                      I.  08 

IO 

1.  01 

3                0.68 

5 

O.6o 

1-5                 1.69 

2 

o-43 

1.29              2.50 

i-5 

0.47 

i.o            4.9 

I.O 

0.63 

0.98          7.0 

0.8 

0.74 

i.o            8.0 

0.51 

1.  00 

1.03         10.  o 

0.25 

2  .OO 

0.29 

5-oo 

1  acetate.                     t  Saturated 

with  water 

'. 

ETHYL    ACETATE  136 

SOLUBILITY  OF  ETHYL  ACETATE  IN  AQUEOUS  ETHYL  ALCOHOL,  METHYL 
ALCOHOL,  AND  ACETONE  MIXTURES  AT  20°. 

(Bancroft  —  Phys.  Rev.  3,  122,  131,  '95-' 96.) 

In  Ethyl  Alcohol. 

Per  i  cc..C2H5OH. 

„_       TT    S\    Or  CC. 

cc.  i^u.*     CH3COOC2He.t 

10  0.25 

8  0.27 

4  0.35 

2  I  -O2 

I .06  2  .  50 

0.65  5-0 

0-54  7-0 

0.44        10.0 


ioo  cc.  H2O  dissolve  7.26  g.  ethyl  acetate  at  28°. 

(Euler  —  Z.  physik.  Chem.  31,  360,  '99.) 

ioo  cc.  H2O  dissolve  9.26  cc.  ethyl  acetate  at  20°. 
ioo  cc.  ethyl  acetate  dissolve  2.94  cc.  water  at  20°. 

ETHYL    BUTYRATE    C3H7COOC2H5. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ETHYL  ALCOHOL  MIXTURES 

AT    20°. 

ioo  g.  H2O  dissolve  0.5  g.  ethyl  butyrate  at  22°. 

(Traube  —  Ber.  17,  2304,  '84-) 

ioo  cc.  H2O  dissolve  0.8  cc.  ethyl  butyrate  at  20°.  (Bancroft.) 

ioo  cc.  ethyl  butyrate  dissolve  0.4  —  0.5  cc.  H2O  at  20°. 

Per  5  cc.  ( cc.  H2O  10          6          4          2.96     2.10 

Ethyl  Alcohol  (  cc.  C3H7COOC2H5       0.34    0.96     2.47     4.00    6.0 

ETHYL    FORMATE    HCOOC2H6. 

ioo  grams  water  dissolve  10  grams  ethyl  formate  at  22°.         (Traube.) 

ETHYL    PROPIONATE    C2H5COOC2H5. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  ETHYL  ALCOHOL  MIXTURES. 

(Bancroft.) 

ioo  grams  H2O  dissolve  1.7  grams  ethyl  propionate  at  22°.      (Traube.) 

.1.1  cc.  H2O  to  cause  separation  of  a  second  phase  in 

cc.  rticoi  ixtures  of  the  given  amounts  of  Alcohol  and  3  cc. 

in  Mature.  portions  of  Ethyl  Propionate. 

3  2.32 

6  6.87 

9  J2-35 

12  19.17 

15  27.12 

18  36.84 

21  50.42 

24  oo 


3 

1.42 

39 

53-13 

9 

7.18 

45 

63.60 

i5 

14-13 

57 

90-53 

21 

22.40 

72 

131.0 

27 

31.62 

81 

180.0 

33 

41  .62 

i37  ETHYL    VALERATE 

ETHYL    VALERATE    C4H8COOC2Hfi, 
ETHYL    (Iso)  VALERATE    (CH3)2.CH.CH2COOC2H6. 

SOLUBILITY  OF  EACH  IN  WATER  AND  IN  AQUEOUS  ALCOHOL 
MIXTURES  AT  20°. 

(Bancroft.) 

ioo  cc.  water  dissolve  0.3  cc.  ethyl  valerate  at  25°. 
100  cc.  water  dissolve  0.2  cc.  ethyl  iso  valerate  at  20°. 
ioo  cc.  ethyl  iso  valerate  dissolve  0.4+  cc.  water  at  20°. 

Mixtures  of  Ethyl  Alcohol,  Mixtures  of  Ethyl  Alcohol, 

Ethyl  Valerate  and  Water.  Ethyl  Iso  Valerate  and  Water. 

Per  5  cc.  Ethyl  Alcohol. 

ec. Alcohol*     cc.H2O.t    cc. Alcohol*     cc.H2O.f  ~~*cc  Ethyl      ' 

cc.H20.      IsoVal/rate. 

10  0.15 

8  0.23 

6  o  .46 

5  0.72 

4  1-23 

*  cc.  Alcohol  in  mixture. 

t  cc.  H2O  added  to  cause  the  separation  of  a  second  phase  in  mixtures  of  the  given  amounts  of  alcohol 
»nd  3  cc.  portions  of  ethyl  valerate. 

Di    ETHYL    KETONE    (3  Pentanon)  (C2H5)2CO. 
SOLUBILITY  IN  WATER. 

(Rothmund  —  Z.  physik.  Ch.  26,  433,  '98  ) 

Determinations  made  by  Synthetic  Method,  see  page  9. 

Cms.  Di  Ethyl  Ketone                                       Cms.  Di  Ethyl  Ketone 
t°.     per  ioo  Gms. t°.       per  700  Gms. 

Aq.  Layer.     Ketone  Layer.  Aq.  Layer.     Ketone  Layer. 

20  4.60     ...  ioo  3-68  93 .10 

40  3-43  97-42  120  4.05  90.18 

60  3.08  96.18  140  4.76  87.01 

80  3.20  94-92  160  6.10  83.33 

ETHYL    BROMIDE    C2H5Br. 

SOLUBILITY  IN  ETHER. 

(Parmentier  —  Com pt.  rend.  114,  1002,  '92.) 
t°.  — 13°-  o-  I2-  22.5.  32. 

G.  C2H5Br  per  ioo  gms.  Ether         632         561          462        302         253 
SOLUBILITY  OF  ETHYL  BROMIDE,  ETC.,  IN  WATER. 

(Rex  —  Z.  physik.  Chem.  55,  355,  '06.) 

Grams  per  ioo  Grams  H2O  at: 

Dissolved  Substance.  , * * 

o°.  10°.  20°.  30°. 

Ethyl  Bromide  1.067  0.965  0.914  0.896 

Ethyl  Iodide  0.441  0.414  0.403  0.415 

Ethylene  Chloride  0.922  o .  885  o .  869  o .  894 

Ethylidene  Chloride  o .  656  o .  595  o .  550  o .  540 


ETHYL    CARBAMATE  138 

ETHYL    CARBAMATE    CO(OC2H5)NH,.     (See  also  Urethane,  p.  347.) 
SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  25°. 

(U.  S.  P.) 
Solvent:  Water.  Alcohol.        Ether.        Chloroform.    Glycerine. 

Cms.  CO(OC2H5)NH2  66 

per  100  gms.  solvent     Ioo+  77  33 

ETHYLENE    C2H4. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Bunsen  and  Carius;  Winkler  —  Landolt  and  Bornstein,  Tabellen,  3d  ed.  p.  604,  '06.) 


o 

P. 
O.226 

Q- 
O.O28l 

Solubility  in  Alec 

«.  o             Vols.  C2H4  per 

5 

O.I9I 

0.0237 

L 

ioo  Vols.  Alcohol. 

10 

O.l62 

O-O2OO 

O 

359-5 

15 

0.139 

O.OI7I 

4 

337-5 

20 

O.I22 

0.0150 

10 

308.6 

25 

0.108 

O.OI3I 

15 

288.2 

30 

0.098 

O.OIlS 

20 

271.3 

For  ft  and  q  see  Ethane,  page  133. 
SOLUBILITY  OF  ETHYLENE   IN  METHYL  ALCOHOL  AND   IN  ACETONE. 

(Levi  —  Gazz.  chim.  ital.  31,  II,  513,  '01.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression  /.    See  p.  105. 

t°.        In  Methyl  Alcohol.        In  Acetone.  t°.        In  Methyl  Alcohol.      In  Acetone. 

o     3-3924     4-0652     30     1-8585     i. 8680 
10     2.8831     3-358°     40     1-3432     1.0852 

20       2.3718       2.6278       50       0.8259       0.2772 
25        2. ,1154       2.2500       60       0.3506 

The  formulas  from  which  the  above  figures  were  calculated  are: 

In  Methyl  Alcohol,       /  =  3  .3924  —  0.05083  t  —  o.ooooi  /2. 
In  Acetone,  /  =  4.0652  —  0.06946  /  —  0.000126  t2. 

PATS. 

SOLUBILITY  OP  THE  FATTY  ACIDS  OBTAINED  FROM  SEVERAL  SOURCES 
IN  ALCOHOL  AND  IN  BENZENE. 

(Dubois  and  Fade  —  Bull.  soc.  chim.  [2]  44,  '85.) 


Crude 
Fatty 

A      *J        t 

Gms. 

Fat  per  ioo  ( 
Alcohol  at: 

Jms.  Abs. 

Gms.  Fats 
per  ioo  Gms. 

T>                                               C 

Acid  of: 

o°. 

10°. 

26°. 

Benzene  at  12  , 

Mutton 

2.48 

5-02 

67.96 

14.70 

Beef 

2.51 

6.05 

82.23 

15.89 

Veal 

5.00 

I3-78 

137.10 

26.08 

Pork 

5-63 

11.23 

118.98 

27.30 

Butter 

10.61 

24.81 

158.2 

69.61 

Margarine 

2.37 

4-94 

47-06 

J3-53 

139  FUMARIO    ACID 

FUMARIC    ACID    COOH.CH:CH.COOH. 
MALEIC    ACID    (CH)2(COOH)2. 

SOLUBILITY  IN  WATER. 

(Vaubel  —  J.  pr.  Chem.  [2]  59,  30,  '99.) 

ioo  gms.  water  dissolve  0.672  gram  fumaric  acid  at  165°. 
ioo  gms.  water  dissolve  50.0  grams  maleic  acid  at  100°. 

FURFUROL   C4H3OCHO. 

SOLUBILITY  IN  WATER. 

(Rothmund  —  Z.  physik.  Chem.  26,  475,  '98.) 

Determinations  by  Synthetic  Method,  for  which  see  page  9. 

0      Gms.  C«H3OCHO  per  ioo  Gms.  Gms.  C4H3OCHO  per  ioo  Gms. 

Aq.  Layer.      Furfurol  Layer.  Aq.  Layer.       Furfurol  Layer. 

40  8.2  93.7  ioo     18.9  83.5 

50  8.6  93.0  no     24.0  78.5 

60  9.2  92.0  115     28.0  74.6 

70  10.8  90.7  120     34.4  68.1 

80  13.0  89.0  122.7  (crit.  t.)  51-0 

90  15.5  86.6 

GADOLINIUM    SULPHATE    Gd2(SO4)3.8H2O. 
SOLUBILITY  IN  WATER. 

(Benedicks  —  Z.  anorg.  Chem.  22,  409,  'oo.) 

to  Gms.  Gd2(S04)s  per  ioo  g  Hd  ph 

Gms  H2L). 

o  3.98  Gd2(SO4)3.8H2O 

10  3-3 

14  2.8 

25  2.4 

34.4  2.26 

GALACTOSE    C6H12O6. 

ioo  grams  saturated  solution  in  pyridine  contain  5.45  grams  C6Hi2O, 
at  26°,  density  of  solution  1.0065. 

(Holty  —  J.  Physic.  Chem.  9,  764,  '05  ) 

GALLIC    ACID   CeH^OHa)  (3,  4,  5)  COOH  +H2O. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.;  Bourgoin  —  Ann.  chim.  phys.  [5]  13,  406,  '78.) 

Gms.  CvHeOs.J^O  per  ioo  Gms. 


doivem. 

i>  . 

Solvent. 

Solution. 

Water 

25 

I  .20 

1.18 

Water 

IOO 

33-3 

25.0 

Alcohol  (Abs.) 

23-3 

18.1 

Alcohol  (U.S.P.) 

25 

24.1 

19-3 

Alcohol  90% 

38.8 

18.9 

Ether 

25 

2.56 

2.50 

Glycerine 

25 

8-3 

7.66 

GERMANIUM    DIOXIDE  140 

GERMANIUM    DIOXIDE    GeO2. 

100  gms.  H2O  dissolve  0.405   gm.  GeO2  at  20°,    and  1.07  gms.  at 
100°. 

(Winkler  — J.  pr.  Chem.  [2]  34,  177.  '86;  36.  i?7,  '87.) 

GERMANIUM  (Mono)    SULPHIDE    GeS    and    GERMANIUM    (Di) 
SULPHIDE    GeS2. 
100  gms.  H2O  dissolve  0.24  GeS  and  0.45  gm.  GeS2. 

(Winkler.) 

GLASS. 

For  data  on  the  solubility  of  glass  in  water  and  other  solvents,  see : 

(Cowper  —  J.  Chem.  Soc.  41,  254,  '82;  Emmerling  —  Liebig's  Annalen,  150,  257,  '69;  Bohling  —  Z. 
anal  Chem.  23,  518,  '84;  Kreusler  and  Herzhold  —  Ber.  17,  34,  '84;  Kohlrausch  —  Ber.  24,  3561,  '91; 
Wied  Ann.  44,  577,  '91;  Forster —  Ber.  25,  '92;  Mylius  and  Forster —  Ber.  22,  noo,  '89;  Ber.  25,  70, 
'92;  Wartha  —  Z.  anal.  Chem.  24,  220,  '85,  etc.) 

GLYCOLIC   ACID    CH2OH.COOH. 

SOLUBILITY  IN  WATER. 

(Emich  —  Monatsh.  Chem.  3,  336,  '84.) 
t°.  20°.  60°.  80°.  100°. 

Gms.  CH2OH(COOH) 

per  too  gms.  H20  °'°33  0.235        0.850 

GLUCINIUM    SALTS.     (See  also  Beryllium  p.  63). 

SOLUBILITY  IN  WATER  AND  IN  ACETIC  ACID  SOLUTIONS. 

(Marignac;   Sestini  —  Gazz.  chim.  ital.  20,  313,  '90.) 

Gms.  Anhydrous  Salt 
Salt.  Formula.  Solvent.  ^perioo  Gms.  Solvent.^ 

At  20°.  At  100°. 

Glucinium  potassium  fluoride  G1F2.KF  Water  2.0  52 

sodium  "        GlF2.NaF  «  1.4  2.8 

Glucinium  hydroxide  G1(OH)2  Water  +  CO2  sat.  0.0185  (G1O)    ... 

phosphate  G13(PO4)2.6H2O      2%  CH3COOH    0.055 

10%  0.1725 

GLUTARIO    ACID    (Pyrotartaric)  (CH2)3(COOH)2. 
SOLUBILITY  IN  WATER. 

(Lamouroux  —  Compt.  rend.  128,  998,  '99.) 
t°.  o°.  15°.  20°.  35°.  50°.  65°. 

Gms.  (CH2)3(COOH)2 

per  loo  cc  solution  42-9     5«-7     63.9     79.7     95.7     111.8 

GOLD   Au. 

SOLUBILITY  OF  GOLD  IN  POTASSIUM  CYANIDE  SOLUTIONS. 

(Maclaurin  —  J.  Chem.  Soc.  63,  729,  '93.) 

Gold  disks  placed  in  Nestler  tubes  with  KCN  solutions. 

Grams  Au  Dissolved  in  24  Hours  in  Nessler  Tubes : 


l    1*1     fciGUl 

KCN. 

Full. 

iFull. 

Oxygen 
Passed  in. 

Oxygen  -f 
Agitation. 

O.I 

O.OOI95 

0.00331 

1.0 

0.00162 

O.OO4I8 

0.00845 

0.0l87 

S-o 

0.0032 

0-0046 

0-01355 

0.0472 

20.0 

O.OOI2 

0.00305 

O.OH5 

0.0314 

50.  o 

0-00043 

0.00026 

0.00505 

Q.OIOS 

141  GOLD    CHLORIDE 

GOLD    CHLORIDE    (Auric)    AuCl3. 

SOLUBILITY  IN  WATER,  ETC. 

100  gms.  H2O  dissolve  68  grams  AuCl3. 

AsCl3  and  SbCl3  each  dissolve  about  2.5%  AuCl3  at  15°,  and  22%  at 
1 60°. 

SnCl4  dissolves  about  4%  AuCl3  at  160°,  and  a  trace  at  o°. 

(Lindet  — Bull.  soc.  chim.  [2]  43,  149.  '86.) 

GOLD    PHOSPHORUS    TRI    CHLORIDE    (Aurous)    AuClPCl3. 
100  gms.  PC13  dissolve  i  gram  at  15°,  and  about  12.5  grams  at  120°. 

(Lindet  —  Compt.  rend.  101,  1492,  '85.) 

GOLD  ALKALI  DOUBLE  CHLORIDES. 

SOLUBILITY  OF  SODIUM  GOLD  CHLORIDE,  LITHIUM  GOLD  CHLORIDE, 
POTASSIUM  GOLD  CHLORIDE,  RHUBIDIUM  GOLD  CHLORIDE,  AND 
CAESIUM  GOLD  CHLORIDE  IN  WATER. 

(Rosenbladt  —  Ber.  19,  2537,  '86.) 

Grams  Anhydrous  Salt  per  100  Grams  Solution. 


Il    . 

NaAuCLi. 

LiAuCU. 

KAuCU. 

RbAuCU- 

CsAuCU- 

10 

58.2 

53-1 

27.7 

4-6 

o-5 

20 

60.2 

57-7 

38.2 

9-0 

0.8 

30 

64.0 

62.5 

48.7 

13-4 

i-7 

40 

69.4 

67-3 

59-2 

17.7 

3-2 

50 

77-5 

72.0 

70.0 

22  .2 

54 

60 

90.0 

76.4 

80.2 

26.6 

8.2 

70 

81.0 

31.0 

12.0 

80 

85-7 

35-3 

I6.3 

90 

39-7 

21-7 

100 

44-2 

27-5 

GUAIACOL    C6H4(OH)OCH3  1:2.     GUAIACOL    CARBONATE   C6H4 
(OCH3)O2.CO. 

SOLUBILITY  IN  WATER,  ALCOHOL,  ETC. 

(U.  S.  P.) 

0  Gms.  per  100  Gms.  Solvent. 

Guaiacol.    Guaiacol  Carbonate. 

Water  25  i  .89 

Alcohol  25  ...  2.08 

Chloroform  25  ...  66.6 

Ether  25  ...  7-69 

Glycerine  25  100 

aTriPhenyl    GUANIDINE    C6H6N:C(NHC6H6)2. 

SOLUBILITY  IN  MIXTURES  OF  ALCOHOL  AND  WATER  AT  25°. 

(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  292,  '94.) 
Gms.  Gms. 


Vol.  %     ( 
Alcohol. 

100 

95 
90 

85 

[^jHsN  :C(  NHCfjHfi} 
per  100  Gms. 
Solvent. 

6.23 

3-75 
2.38 

1.58 

(2        Density 
of  Solutions. 

0-8021 

0.8158 
0.8309 
0.8433 

Vol.% 
Alcohol. 

80 

75 
70 
60 

per  100  Gms. 
Solvent. 

1.  06 
0-67 
0.48 
0-22 

5)2       Density 
of  Solutions. 

0.8572 
0.8704 
0.8828 

o  .  9048 

HELIUM 


142 


HELIUM    He. 


SOLUBILITY  IN  WATER. 

(Estreicher  —  Z.  physik.  Chem.  31,  184,  '99.) 

Absorption  Coefficient. 


r.Barometic  Vol.  of 
Pressure.   Water. 

Vol.  of 
He.       «' 

. 

.  . 

0 

.000270 

764 

.0 

73 

•584 

I 

.093 

758 

.0 

73 

•578 

I 

.062 

0 

.000260 

758 

.0 

73 

•597 

I 

.046 

0.000255 

757 

.8 

73 

.641 

I 

.008 

o 

.000246 

758 

•4 

73 

.707 

0 

.996 

0 

.000242 

762 

•3 

73 

•793 

0 

•983 

0 

.000238 

764 

•4 

73 

.897 

0 

•985 

0 

.000238 

764 

•5 

74 

.0167 

0 

.972 

0 

.000234 

762 

.0 

74 

.147 

0 

•957 

0 

.000232 

76! 

•7 

74 

.294 

0 

•947 

0 

.000229 

760 

•9 

74 

.461 

0 

.920 

0 

.000223 

o 

o-5 
5 
10 

15 

20 
25 
30 

35 
40 

45 
5° 
For  q  and  also  Absorption  Coefficient,  see  Ethane,  page  133. 


At  Bar.  Pressure 
Minus  H2O 
Vapor  Tension. 

At  760  mm. 
Pressure. 

O.OI5O 

O.OI49 
0.0144 

O.OI49 
0.0146 

0.0142 

0.0144 

0.0137 

0.0140 

0-0135 

0.0139 

0.0133 
0.0133 
O.OI3I 

0.0137 
0-0138 
0-0138 

0.0129 

0.0139 

O.OI27 

O.OI4O 

O.OI24 

O.OI4O 

HEXANE    C6H14. 

SOLUBILITY  IN  METHYL  ALCOHOL. 

(Rothmund  —  Z.  physik.  Chem.  26,  475,  '98.) 

Determined  by  Synthetic  Method,  see  page  9. 

Gms.  Hexane  per  100  Gms.  Gms.  Hexane  per  TOO  Gms. 


10 

20 
30 


Alcoholic 
Layer. 

26.5 

31-6 
38-3 


Hexane 
Layer. 

96.8 

95-9 
93-7 


Hexane 
Layer. 


t    •  Alcoholic 

Layer. 

35  43 -6          91-2 

40  52-7          85.5 

42.6(crit.  t.)  68.9 


:  Solutions. 

C9H9N03. 

KC9H8N03. 

I  .002 

O.Ol82 

O 

1.003 

0.0163 

O-OII 

I.OOS 

0.0183 

0-071 

I  -O22 

0.0234 

0.254 

I  .114 

0.064 

I.36 

I.I82 

O.I3I 

2.21 

I  .  192 

0.147 

2.32 

i  .  195* 

0-153 

2.40 

i  .201 

0-133 

2.50 

1.239 

0.084 

3-oi 

1.282 

0.068 

3-57 

1.282 

0-065 

3-58 

i  .  276 

0.031 

3-56 

1.277 

p.  oi  i 

3-55 

I-m 

.O.OO 

3-56 

Solid 
Phase. 


HIPPURIO    ACID    C6H6CONH.CH2COOH. 

SOLUBILITY  IN  AQ.  POTASSIUM  HIPPURATE  SOLUTIONS  AT  20°. 

(Hoitsema  —  Z.  physik.  Chem.  27,  317,  '98.) 
Grams  per  Liter  Solution. 
C9H9NO3.     KCgHgNOs. 

3.276         o.o 

2.919  2.39 

3.278  15.43 

4.I9I  55.18 

11-47  295.4 

23.46  480-1 

26.32  504.1 

27.40  521.4 

23.82  543.1 

15.04  654.0 

12. 18   775.7 
II. 60  777.8 

5-55   773-4 
1.917  771.3 

•••   773-4 


C9H9N03  + 


C9H9N03.KC9H8N03.H2O 
+  KC9H8N03 


143  HOMATROPINE  HYDRO- 

BROMIDE 

HOMATROPINE    HYDROBROMIDE    C16H21NO3.HBr. 
SOLUBILITY  IN  WATER,  ETC. 

(U.  S.  P.) 

100  grains  water  dissolve  17.5  grams  salt  at  25°. 
100  grams  alcohol  dissolve  3.08  grams  salt  at  25°,  and  11.5  grams 
at  60°. 

100  grams  chloroform  dissolve  0.16  gram  salt  at  25°. 


HYDRASTINE     C21H21NO6.         HYDRASTINE    HYDROCHLORIDE 
CUHUNO,.HC1. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.;  Muller — Apoth.-Ztg.  18,  249,  '03.) 

Gms.  C2iH2iNC>6  per  100  Gms.  Gms.  per  100  Gms. 

Solvent.  Solution. Solvent.  Solution  at  i8°-22°. 

'  At  i8°-22°.  *~       At  80°.  C2lH2lNO6.    C11H11NO2.HCr. 

Water  0.0033  °-025  Ether  0.51        0.078  (25°) 

Alcohol  0.74(25°)  5.9(60°)  Ether  +  H2O  0.80 

Benzene  8.89  ...  Chloroform  100+       0-35(25°) 

Acetic  Ether  4.05  ...  CC14  o.  123 

Petroleum  Ether  0.073 


HYDRAZINE    SULPHATE    N2H4.H2SO4. 

100  grams  water  dissolve  3.055  grams  N2H4.H2SO4  at  22°. 

(Curtius  and  Jay  —  J.  pr.  Chem.  [2]  39,  39,  '89.) 

HYDROBROMIC    ACID    HBr. 

SOLUBILITY  IN  WATER. 

(Roozeboom  —  Z.  physik.  Chem.  2,  454,  '88;  Rec.  trav.  chim.  4,  107,  '85;  5,  358,  '86;  see  also  Pickering 
—  Phil.  Mag.  [5]  36,  119,  '93-) 

Gms.HBr  KffiolvedjCat  760-7651^.)  Gms  HBr  Dissolved  at 

/3.  Lower  Pressures  per  100 

Gms.  H2O. 

175.0  (10  mm.) 

611.6 

581 .4     108.5  (5  mm.) 

532-1 
468.6 
406.7 
344.6 


t°. 

per  100  L 

rms. 

'      Water. 

Solution. 

-  2.5 

255-0 

7I-83 

—  15 

239.0 

70.50 

o 

221  .2 

68.85 

+  10 

210-3 

67.76 

15 

204-0 

67.10 

25 

193.0 

65.88 

5° 

171  .5 

63.16 

75 

ISO'S 

60.08 

100 

130.0 

56-52 

For  /3  see 

Ethane,  page 

!33- 

HYDROCHLORIC    AGID  144 

HYDROCHLORIC    ACID    HC1. 

SOLUBILITY   IN   WATER  AT  DIFFERENT  TEMPERATURES  AND 
PRESSURES. 

(Deicke;  Roscoe  and  Dittmar  —  Liebig's  Ann.  112,  334,  '59;  below  o°,  Roozeboom  —  Rec.  trav. 

chim.  3,  104,  '84.) 

At  Different  Temperatures  and  760  mm.  Pressure.  At  Different  Pressures  and  o°. 


t°. 

cc.  HC1  per 
ioocc.H2O. 

Density. 

Cms.  HC1  per  Gms.  HC1  per 
100  g.  Sol.        100  g.  H2O. 

Pressures.* 

Gms.  HClper 
100  g.  H2O. 

0 

525-2 

1.2257 

45-15 

82.31 

60 

6l.3 

4 

497-7 

I  .2265 

44  -36 

79-73 

100 

65-7 

8 

480.3 

1.2185 

43-83 

78.03 

150 

68.6 

12 

471-3 

I  .2148 

43-28 

76.30 

200 

70.7 

14 

462.4 

1.2074 

42.83 

74-92 

300 

73-8 

18 

451.2 

I  .  2064 

42-34 

73-41 

4OO 

76-3 

23 

435-o 

I.20I4 

41-54 

71.03 

500 

78.2 

30 

40.23 

67-3 

600 

80.0 

40 

,  38-68 

63-3 

750 

82.4 

So 

37-34 

59-6 

IOOO 

85.6 

60 

35-94 

56.1 

1300 

89-5 

*  Pressures  in  mm.  Hg  minus  tension  of  H2O  vapor. 


At  a  pressure  of  760  mm.       At  pressures  below  and  above  760  mm. 

t°.               q.                     t°.           q.                               t°.  mm.  Pressure.          q. 

-24            IOI.2             -15       93.3                        -23.8  ...                 84.2 

—  21          98.3         —io    89.8                —2i  334          86.8 

—  18.3      96.0        —  5    86.8                —19  580          92.6 
— 18          95.7              o    84.2                 — 18  900          98.4 

-17.7  1073  101.4 
For  value  of  q,  see  Ethane,  page  133. 


SOLUBILITY  OF  HYDROCHLORIC  ACID  GAS  IN  METHYL  ALCOHOL,  ETHYL 
ALCOHOL,  AND  IN  ETHER  AT  760  MM.  PRESSURE. 

(de  Bruyn  —  Rec.  trav.  chim.  u,  129,  '92;  Schuncke  —  Z.  physik.  Chem.  14,  336,  '94.) 

Grams  HC1  gas  per  100  Grams  Solution  in: 

» 

)H.  C2H6OH.  (C2 

-10  e4.6  ...  37.51  (-9.2°) 

-  5 
o 

+  5 
io 

15 

20 

25 
30 


CH3OH. 

C2H6OH. 

(C2H6)20. 

^4.6 

37-51  ( 

37-o 

5J-3 

45-4 

35-6 

44-2  (6.5°) 

33-i 

42.7(11-5°) 

30.35 

27  .62 

47  -0  (18°) 

41  .0 

24.9 

43-0(31-7°) 

40.2  (23.5°) 

38.1  (32°) 

22.18 
19.47 

145  HYDROFLUORIC    ACID 

HYDROFLUORIC    ACID    HF. 

100  grams  H2O  dissolve  in  grams  HF  at  35°. 

(Metzner  —  Compt.  rend.  119,  683,  '94.) 

HYDRIODIO    ACID    HI.     IODIO    ACID    HIO3. 

For  determinations  of  the  freezing  points  of  aqueous  solutions  of  HI, 
and  isolation  of  the  several  hydrates  at  temperatures  below  o°,  see 
Pickering — Ber.  26,  2307,  '93. 

SOLUBILITY  OF  IODIC  ACID  AND  ITS  MODIFICATIONS  IN  WATER. 

(Groschuff  —  Z.  anorg.  Chem.  47,  343,  '05.) 


Grams  per  100 
Gms.  Solution. 

Gram  Mols.  I2OB 
per  100  Gm.  Mols. 

Solid 

HIO3. 

I208. 

H20. 

Solution. 

Phase. 

-14 

72.8 

69.1 

12.  1 

10.8 

Ice  +  HIOa 

0 

74-1 

70-3 

12.8 

"•3 

HI03 

16 

75-1 

71.7 

13-7 

12.0 

u 

40 

77-7 

73-7 

IS-1 

13.2 

a 

60 

80.0 

75-9 

17.0 

14-5 

a 

80 

82.5 

78-3 

19.4 

I6.3 

« 

85 

83.0 

78.7 

20-0 

I6.7 

« 

IOI 

85.2 

80.8 

22.8 

18.6 

« 

no 

86.5 

82.1 

24.7 

19.8 

HIO,  +  HL.O, 

125 

87.2 

82.7 

25-9 

20.  6 

HI308 

140 

88.3 

83.8 

27.9 

21.8 

n 

1  60 

9o-5 

85-9 

32.8 

24-7 

tl 

f— 
Aq. 
Solution. 

27.73%  HN03 
Solution. 

40.88%  HNOa 
Solution. 

74-1 

18.0 

9-0 

75-8 

21  .0 

IO-O 

77-7 

27.0 

14.0 

80.0 

38.0 

18.0 

SOLUBILITY  OF  IODIC  ACID  IN  NITRIC  ACID. 

(Groschuff.) 
Grams  HIOs  per  100  Grams. 


O 
2O 
40 
60 

HYDROGEN    H.  SOLUBILITY  IN  WATER. 

(Winkler  —  Ber.  24,  99,  '91;  Bohr  and  Bock  —  Wied.  Ann.  44,  318,  '91;  Timofejew  —  Z.  physik. 

Chem.  6,  147,  '90.) 

t°.                ft'.            _  L  _  ^                     ft.  q. 

o   0.0214  0.0214  0.000193 

5   0.0203  0.0209  —  0.0241  0.0204  0.000184 

10   0.0193  0-0204  —  0.0229  0.0195  0.000176 

15   0.0185  0.0200  —  0.0217  0.0188  0.000169 

20    0.0178   0-0196  -  0.0205  0.0182  0.000162 

25       0.0171     0.0193   —   0.0191  0.0175  0.000156 

30      0.0163         ...                ...  0.0170  0.000147 

40       0.0153         ...                ...  0-0164  0.000139 

50      0.0141        ...               ...  0.0161  0.000129 

60      0.0129        ...               ...  0.0160  0.000119 

80      0.0085        ...               —  0.0160  0.000079 

100      o.oooo        ...               ...  0.0160  o-oooooo 

/  =  Ostwald  Solubility  Expression,  see  page  105.  For  /?',  ft,  and  q> 
see  Ethane,  page  133. 


HYDROGEN 


146 


SOLUBILITY   OP   HYDROGEN   IN  AQUEOUS   SOLUTIONS   OF  ACIDS   AND 

BASES  AT  25°. 

(Geffcken  —  Z.  physik.  Chem.  49,  268,  '04.) 


Gram  Equiv. 
Acids  and 


Solubility  of  H 


Ostwald  Expression)  in  Solutions  of: 


per  Liter.  HC1' 

o.o  0.0193 

0.5  0.0186 

i.o  0.0179 

2 .O  O .Ol68 

3.0  0.0159 


4.0 


HN03. 
0.0193 
0.0188 
0-0183 
0.0174 
0-0167 

0.0160 


iH2S04.   CHgCOOH.  CH2C1COOH.    KOH.         NaOH. 
0.0193      0.0193 
O.OI92      0-0189 


0.0193 
0.0185 
0.0177 
0.0163 
0.0150 
O.OI4I 


O.OI9I 
0.0188 

0.0186 
0.0186 


0.0186 
0.0180 


0.0193 
0.0167 
0.0142 


0.0193 
0.0165 
0.0139 
0.0097 
0.0072 
0.0055 


The  above  figures  for  the  concentrations  of  acids  and  bases  were 
calculated  to  grams  per  liter,  and  these  values  with  the  corresponding 
/25  values  for  the  solubility  of  hydrogen  plotted  on  cross-section  paper. 
From  the  resulting  curves  the  following  table  was  read. 


Grams  Acids 
and  Bases 
per  Liter. 

0 
20 

40 

60 
80 
IOO 

150 

2OO 
250 

Solubility  of  H 

(fe6  = 

Ostwald  Expression)  in  Solutions  of: 

0 
0 
0 
0 
0 
0 

HC1. 

.0193 
.0185 
.0179 
.0173 

.0167 
.0160 

HN03. 
0.0193 
0-0189 

0.0186 
0.0183 
0.0180 
0.0179 
0.0171 
0.0165 
0.0160 

*H2S04. 
0.0193 

0.0186 
0.0180 
0.0174 
0.0168 
0.0162 
0.0148 
0.0140 

CH3COOH. 
0.0193 
O.OI92 
O.OI9I 
O.OI9O 
0.0189 
0.0189 
0.0188 

0.0186 
0.0184 

CH2C1COOH 

0.0193 

0.0191 
0.0190 
0.0188 
0.0187 
0.0185 
0.0182 
0.0179 

0 
0 
0 
0 

KOH. 

.0193 

.0172 

•0153 

•o^S 

NaOH. 
0.0193 
0.0l65 
O.OI4O 
O.OII7 
O.OO97 
0.0082 
0.0058 

For  Ostwald  Solubility  Expression,  see  page  105. 


SOLUBILITY   OF   HYDROGEN   IN  AQUEOUS   SOLUTIONS   OF  AMMONIUM 

NITRATE  AT  20°. 

(Knopp  —  Z.  physik.  Chem.  43,  103,  '04.) 


p- 

Normality 
(per  1000  Gms.) 
H2O. 

Molecular 
Concentra- 
tion. 

Absorption 
Coefficient 
of  Hydrogen. 

Density 
of  Solutions. 

o.oo 

O-OO 

o.oo 

0.0188 

1.037 

o  .  1308 

0.002352 

0.01872 

1.0027 

2  .167 

0.2765 

0.004956 

0.01845 

1.0072 

3-378 

0.4363 

0.007799 

0.01823 

I  -OI22 

4-823 

0-6333 

0.011280 

0.01773 

I.OI82 

6-773 

o  .  9069 

0.016447 

0.01744 

1.0262 

1.550 

1.6308 

0.028525 

0.01647 

1.04652 

147 


HYDROGEN 


SOLUBILITY    OP    HYDROGEN    IN    AQUEOUS    SOLUTIONS    OF 

CHLORIDE. 

(Braun  —  Z.  physik.  Chem.  33,  735,  'oo.) 


BARIUM 


Cms.  BaCl2 

Coefficient  of  Absorption  of  Hydrogen  at  : 

A 

per  100  Gms. 
Solution. 

5°. 

10°. 

IS°- 

20°. 

25°. 

O-OO 

0.0237 

O-022I 

0.0206 

0.0191 

0.0175 

3-29 

O-02II 

0-0198 

0.0185 

0.0172 

0.0157 

3-6 

0.02O9 

O.OI97 

0.0184 

0.0170 

0.0156 

6-45 

0-0196 

0.0186 

0.0173 

0.0161 

0.0147 

7.00 

O.OI94 

0.0183 

0.0172 

0.0159 

0.0146 

SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  CALCIUM  CHLOR- 
IDE, MAGNESIUM  SULPHATE,  AND  LITHIUM  CHLORIDE  AT  15°. 

(Gordon  —  Z.  physik.  Chem.  18,  14,  '95.) 

Coefficient  of  Absorption  of  hydrogen  in  water  at  15°  =  0.01883. 
In  Calcium  In  Magnesium  In  Lithium 


Chloride. 


Sulphate. 


Chloride. 


Gms. 
CaCl2 

G.M. 
CaCl2 

Absorption 
Coefficient 

Gms. 
MgS04 

G.M. 
MgS04 

Absorption 
Coefficient 

Gms. 
LiCl 

G.M. 
LiCl 

Absorption 
Coefficient 

per 
too  g.  Sol. 

per 
Liter. 

of  H. 

per 
zoo  g.  Sol. 

per 
Liter. 

of  H. 

per 

100  g.  Sol. 

per 
Liter. 

of  H. 

3-47 

0.321 

0.01619 

4-97 

o-433 

0.01501 

3-48 

0-835 

0.01619 

6.  10 

0.578 

0.01450 

10.19 

0.936 

0.01159 

7-34 

1.800 

0.01370 

"•33 

I.  122 

0.01138 

23.76 

2.501 

0.00499 

14.63 

3-734 

0.0099 

i7-52 

I.I827 

0.00839 

26.34 

2.962 

0.00519 

For  definition  of  Coefficient  of  Absorption,  see  page  105. 

SOLUBILITY   OF   HYDROGEN   IN   AQUEOUS   SOLUTIONS   OF   POTASSIUM 
CARBONATE,  CHLORIDE,  AND  NITRATE  AT  15°. 

(Gordon.) 


In  Potassium 

In  Potassium 

In  Potassium 

Carbonate. 

Chloride. 

Nitrate. 

Gms. 
K2C03 

G.M. 
K2C03 

Absorption 
Coefficient 

Gms. 
KC1 

G.M. 
KC1 

Absorption 
Coefficient 

Gms. 
KN03 

G.  M. 
KN03 

Absorption 
Coefficient 

per 
100  g.  Sol. 

per 
Liter. 

of  H. 

per 

100  g.  Sol. 

per 
Liter. 

of  H. 

per 
100  g.Sol. 

Liter. 

of  H. 

2.82 

0.209 

0.01628 

3.83 

0.526 

0.01667 

4-73 

0.482 

0.01683 

8-83 

0.690 

0.01183 

7.48 

1.051 

0.01489 

8.44 

0.879 

0-01559 

16.47 

1.376 

0.00761 

12.13 

i-755 

0.01279 

16.59 

1.820 

0.01311 

24.13 

2.156 

0.00462 

19.21 

2.909 

O.OIOI2 

21.46 

2.430 

O.OIlSo 

4I.8l 

4.352 

O.OOl6o 

22.92 

3-554 

0.00892 

SOLUBILITY    OF    HYDROGEN    IN   AQUEOUS    SOLUTIONS    OF    POTASSIUM 
CHLORIDE  AND  NITRATE  AT  20°. 

(Knopp  —  Z.  physik.  Chem.  43,  103,  '04.) 


In  Potassium  Chloride. 


In  Potassium  Nitrate. 


p> 

Normality 
(per  looo 
g.  H20). 

Absorption 
Coefficient. 

Density 
of 
Solutions. 

P- 

Normality 
(per  looo 
g.  H20). 

Absorption          De"sity 
Coefficient.       Solutions 

1.089 

0 

•1475 

0-01823 

I 

.0052 

I 

224 

O 

.1245 

0.01835 

.0059 

2  .123 

0 

.2907 

0.01757 

I 

.OIl8 

2 

094 

0 

.2114 

o.  01818 

.0113 

4.070 

0 

.5687 

o.  01661 

I 

.0243 

4 

OIO 

0 

.4127 

0-01785 

.0236 

6-375 

0 

.9127 

O.OI53I 

I 

•0394 

5 

925 

0 

.6225 

0.01743 

•0359 

7.380 

I 

.0682 

0.01472 

I 

.0460 

7 

742 

0 

.8293 

0-01667 

.0477 

13.612 

2 

.1222 

0.01255 

I 

.0875 

13 

.510 

I 

•5436 

0.01436 

.0865 

HYDROGEN 


148 


SOLUBILITY   OP   HYDROGEN    IN   AQUEOUS    SODIUM   CARBONATE   AND 
SULPHATE  SOLUTIONS  AT  15°. 

(Gordon.) 

In  Sodium  Carbonate.  In  Sodium  Sulphate. 


Gms.  NaizCOs      G.M. 
per  100  Gms.      Na2COa 

Absorption 
Coefficient 

Gms.  Na2SO4       G.  M. 
per  100  Gms.      Na2SO4 

Absorption 
Coefficient 

Solution.        per  Liter. 

of  H. 

Solution.         per  Liter. 

of  H. 

2.15            O.2O7 

0-01639 

4-58        Q-33S 

O.OI5I9 

8.64           0.438 

0.01385 

8.42        0.638 

0.0154 

11.53        1.218 

0.00839 

16.69        1.364 

0.00775 

SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

CHLORIDE. 

(Braun;  Gordon.) 


Gms.NaCl 

Coefficient  of  Absorption  of  Hydrogen  at: 

per  100  Gms. 
Solution. 

5°- 

10°. 

15°. 

20°. 

25°. 

1.25 

0.0218 

O.O2O5 

O.OI9I 

0.0177 

0.0162 

3.80 

0.0198 

0.0188 

O.OI76 

O.0l62 

0.0148 

4.48 

0.0192 

0.0l82 

O.OI7I 

O.OI59 

0.0143 

6.00 

0.0184 

0.0175 

0.0164 

0.0153 

0.0138 

14-78 

0.0093 

23.84 

0.00595 

SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 

NITRATE. 
In  Sodium  Nitrate  at  20°.  In  Sodium  Nitrate  at  15°. 

(Knopp.)  (Gordon.) 


r~ 

Normality 

Absorption 

\ 
Density 

Gms.NaNOa 

G.M. 

Absorption 

p- 

(per  1000 

Coefficient 

of 

per  loo  Gms. 

NaNO3 

Coefficient 

Gms.  H20). 

of  H.                 S 

qlutions. 

Solution. 

per  Liter. 

of  H. 

1.041 

0.1236 

0.01839 

.0052 

5-57 

0.679 

0.01603 

2  .192 

0.2634 

0.01774 

.0130 

II  .16 

I-4I3 

0.0137 

4-405 

0.5416 

0.01694 

.0282 

19.77 

2.656 

O.OIO52 

6.702 

o  .  8442 

O.OI5l8 

.O44II 

37-43 

5-7II 

0.00578 

12.637 

1-7354 

O.OI3O 

.08667 

SOLUBILITY  OF  HYDROGEN  IN  ALCOHOL. 

(Timofejew  —  Z.  physik.  Chem.  6,  147,  '90.) 


o 

6.2 

13-4 

18.8 

Coefficient  of  Abs.  in 
08.8%  Alcohol. 

0.0676 
0.0693 
0.0705 
O.O74O 

4 
18.8 

Coefficient  of  Abs.  in 
99-7%  Alcohol. 

0.0749 
0.0740 


SOLUBILITY    IN  AQUEOUS  ALCOHOL  SOLUTIONS   AT  20°  AND  760  MM. 

PRESSURE. 

(Lubarsch  —  Wied.  Ann.  [2]  37,  525,  '89.) 


Wt.  %  Alcohol. 

o.oo 

Vol.  %  Absorbed  H. 

i-93 

Wt.  %  Alcohol. 
28.57 

Vol.  %  Absorbed  H. 
1.04 

9.09 
16.67 
23.08 

i-43 
i  .29 
1.17 

33-33 
50.0 
66.67 

I.I7 
2.02 

2-55 

149 


HYDROGEN 


SOLUBILITY  OF  HYDROGEN  IN  AQUEOUS  SUGAR  SOLUTIONS  AT  15°. 

(Gordon  — Z.  physik.  Chem.  18,  14,  '95.) 


Gms.  Sugar  per 
zoo  Gms.  Solution. 

16.67 
30.08 

47 -65 


Gm.  Mols.  Sugar 
per  Liter. 

0.520 

0-993 
1.699 


Absorption 
Coefficient  of  H. 

0-01561 
0.01284 
0.00892 


SOLUBILITY  OF  HYDROGEN  IN  WATER  AND  IN  ORGANIC  SOLVENTS. 
Results  in  terms  of  the  Ostwald  Expression,  see  page  105. 

(Just  —  Z.  physik.  Chem.  37,  359,  '01.) 
Solvent.  /2s-  /so- 

Amyl  Acetate  0.0774  0.0743 

Xylene  0.0819  0.0783 

Ethyl  Acetate  0.0852  0.0788 

Toluene  0.0874  0.0838 

Ethyl  Alcohol  (98.8%)  o.  0894  o.  0862 

Methyl  Alcohol  0.0945  0.0902 

Iso  Butyl  Alcohol  0.0976  0.0929 


Solvent. 

Water 
Anilin 
Amyl  Alcohol 
Nitro  Benzene 
Carbon  Bisulphide 
Acetic  Acid 
Benzene 
Acetone 

0. 

o. 

0. 
0. 
0. 
0. 
0. 
0. 

fa. 

0199 
0285 
0301 
0371 

0375 
0633 
0756 
0764 

0. 

o. 

0. 

o. 

0. 
0. 
0. 
0. 

feo- 

0200 

0303 
0353 
0353 
0336 

0617 

0707 
0703 

SOLUBILITY  OF  HYDROGEN   IN   CHLORAL  HYDRATE   SOLUTIONS 


AT    20". 

(Knopp.) 

p- 

Normality  (per 
1000  Gms.  H2O). 

Molecular 
Concentration. 

Absorption 
Coefficient  of  H. 

Density 
of  Solutions. 

4.91 

0.310 

0.005594. 

0-01839 

I  .O2O2 

7.69 

0.504 

0-008992 

0.01802 

I  .0320 

14.56 

1.030 

0.0l8223 

O.OI7I2 

I  .0669 

29.50 

2-530 

0.04360! 

O.OI542 

1.1466 

38.42 

3-770 

0.063647 

0.01440 

1.1982 

49-79 

6.000 

0.097493 

0.01353 

1.2724 

63.90 

10.700 

o.  161660 

0.01307 

1-3743 

SOLUBILITY  OF  HYDROGEN  IN  PROPIONIC  ACID  SOLUTIONS. 

(Braun.) 


G.  CaHsCOOH 

Coefficient  of  Absorption  of  Hydrogen  at: 

per  100  Oms. 
Solution. 

5°- 

10°. 

15°. 

20°. 

25°. 

2  .63 

0.02245 

0.0214 

O-O2OO 

0.0188 

0.0172 

3-37 

0.0222 

0.0212 

O.OI99 

0.0187 

0.0171 

5-27 

O.O224 

O-02I2 

0.0198 

0.0184 

0.0171 

6.50 

0.0218 

O.O2O9 

0.0193 

0.0183 

0.0169 

9.91 

0.0213 

0.0203 

O.OI9I 

0.0178 

0.0160 

SOLUBILITY  OF  HYDROGEN  IN  PETROLEUM. 

(Griewasz  and  Walfisz  —  Z.  physik.  Chem.  i,  70,  '87.7 

Coefficient  of  absorption  at  20°  =  0.0582,  at  10°  =  0.0652. 


HYDROGEN    SULPHIDE  150 

HYDROGEN    SULPHIDE   H2S. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL  AT  t°  AND  760  MM.  PRESSURE. 

(Bunsen  and  Carius;  Fauser  —  Math,  u  Natur.  W.  Ber.  (Ungarn.)  6,  154,  '88.) 


In  Water. 


/  

t     . 

i  Vol 

.  H20  Absorbs 

ft. 

3- 

o 

5 

4 

3 

•37 
•97 

Vols.  H2S(ato°  and 

U 

760  mm.)  4 

4 

.686 
.063 

0 
0 

.710 
.615 

10 
J5 

20 
25 

3 
3 

2 
2 

•59 
•23 
.91 
.61 

U 

3 
3 

2 

.520 
.056 
.672 

0 
0 
0 

•530 
•458 
•398 

30 

35 
40 

2 
2 
L 

•33 

.08 
.86 

: 

In  Alcohol. 

i  Vol.  Alcohol  Absorbs 
17.89  Vols.  H2S(at  o°  and  760  mm .) 

14-78 
11-99 

9-54 
7.42 
5-96  (24°) 


For  ft  and  q  see  Ethane,  page  133. 


SOLUBILITY  OF  HYDROGEN  SULPHIDE  IN  AQUEOUS  SALT  SOLUTIONS 


AT    25°. 
(McLauchlan  —  Z.  physik.  Chem.  44   6cs,  '03.) 


NOTE.  —  The  original  results  are  given  in  terms  of  -r  which  is  the 

LO 

iodine  titer  (I)  of  the  H2S  dissolved  in  the  salt  solution  divided  by  the 
titer  (/0)  of  the  H2S  dissolved  in  pure  water.  These  figures  were  multi- 
plied by  2.  6  1  (see  25°  results  in  preceding  table)  and  the  products 
recorded  in  the  following  table  as  volumes  of  H2S  absorbed  by  i  vol. 
of  aqueous  solution. 


Solution. 

Grams  Salt 
per  Liter. 

I          Vols.  H2S 
lo.      per  i  Vol.  Sol 

.       Solution.      G-.S.U 

I         Vols.  H2S 
/0.      per  i  Vol.  So* 

n  NH4Br 

98, 

,o 

I.OO 

2.61 

n 

KBr 

119 

.0 

0. 

945 

2-47 

n  NH4C1 

53- 

4 

0.96 

2.40 

n 

KC1 

74 

•  5 

O. 

853 

2.  22 

n  NH4NO3 

80 

,o 

0.99 

2.58 

n 

KN03 

101 

.0 

0. 

913 

2.38 

Jn  (NH4)2S04 

33 

0 

0.82 

2.14 

in 

K2SO4 

43 

•  5 

0. 

78 

2.O4 

in  (NH4)2S04 

16. 

5 

o.  91 

2.37 

In 

K2S04 

21 

•7 

o. 

89 

2.32 

n  NH4C2H3O2 

77. 

j 

1.09 

2.84 

n 

KI 

166 

.0 

0. 

98 

2.56 

n  (NH2)2CO 

60, 

,  i 

1.02 

2.66 

n 

NaBr 

103 

.0 

o. 

935 

2.44 

\n  HC1 

18. 

22 

0-975 

2-54 

n 

NaCl 

58 

•5 

0. 

847 

2.21 

in  H2SO4 

24. 

52 

0.905 

2.36 

in 

NaCl 

29 

.2 

o. 

93 

2.42 

n  C4H606 

150- 

0 

0.944 

2.46 

n 

NaNO3 

85 

.0 

0. 

893 

2.32 

3n  C4H606 

45o. 

o 

0.858 

2.  24 

in 

Na2S04 

35 

•  5 

0. 

73 

1.90 

Pure  C3H5(OH)3 

1000.  0 

0.863 

2.26 

in 

Na2S04 

i7 

.8 

0. 

89 

2.32 

HYDROQUINONE    C6H4(OH)2  i  :4,  also  Resorcin  C6H4(OH)2  i  :3  and 
Pyrocatechin    C6H4(OH)2  1:2. 

SOLUBILIT.Y  IN  WATER. 

(Vaubel  —  J.  pr.  Chem.  [2]  59,  30,  '99.) 

TOO  grams  solution  contain  6.7  grams  hydroquinone  at  20°.  Sp.  Gr. 
of  sol.   =  1.012. 

100  grams  solution  contain  63.7  grams  resorcin  at  20°. 
TOO  grams  solution  contain  31.1  grams  pyrocatechin  at  20°. 


I5i  HYDROQUINONE 

SOLUBILITY   OF   HYDROQUINONE  IN   SULPHUR   DIOXIDE   IN  THE 
CRITICAL  VICINITY. 

(Centnerswer  and  Teletow  —  Z.  Electrochem.  9,  799,  '03.) 

Determinations  made  by  the  Synthetic  Method,  for  which  see  Note, 
page  9. 

^o     Gms.  Hydroquinone         ^0       Gms.  Hydroquinone       to         Gms.Hydroquinone 
per  IOQ  Gms.  Sol.  per  100  Gms.  Sol.  '     per  100  Gms.  Solution. 

63       0.89       117.6     4.46       136.7     10.31 

73.5        1.22  123.3        5 -66  141-4        13-3 

89.2  2.l8  134.2  8.31  145-0  14-9 


HYDROXYLAMINE   NH2(OH).  HYDROXYLAMINE   HYDRO- 
CHLORIDE  NH2(OH).HC1. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(de  Bjxiyn  —  Rec.  trav.  chim.  n,  18,  '92;  Z.  physik.  Chem.  10,  783,  '92.) 

Grams  NH2OH  Grams  NH2(OH).HC1 

Solvent.  t°.  per  100  Gms.        t°.  per  100  Gms. 

Solution.  Solvent. 

Methyl  Alcohol  (abs.)  5°  35-o        T9-75         16.4 

Ethyl  Alcohol  (abs.)  15°  15.0         19-75          4-43 

Ether  (dry)  (b.  pt.)           1.2 

Ethyl  Acetate  (b.  pt.)          1.6 

For  densities  of  NH2(OH).HC1  solutions,  see  Schiff  and  Monsacchi  — 
Z.  physik.  Ch.  21,  277,  '96. 


HYOSCYAMINE    C17H21NO3. 

SOLUBILITY  IN  SEVERAL  SOLVENTS  AT  i8°-22°. 

(Miiller  — Apoth.-Ztg.  18,  249,  '03.) 

Gms.  C,7H21NO3  Gms.Ci7H2iN 

Solvent.  per  100  Gms.  Solvent.  per  I0°  Gms. 

Solution.  Solution. 

Water  °-355  Chloroform  100+ 

Ether  2.02  Acetic  Ether  4-903 

Ether  sat.  with  H2O     3.913  Petroleum  Ether  0.098 

Water  sat.  with  Ether  3  .125  Carbon  Tetra  Chloride    0.059 
Benzene                          o .  769 


HYOSCINE    HYDROBROMIDE,  etc. 

SOLUBILITY  IN  SEVE.RAL  SOLVENTS  AT  25°. 

(U.  S.  P.) 
.  Grams  per  100  Grams  Solvent. 


Solvent.                      Hyoscine 
Hydrobromide 
C,7H21N04.HBr.3H20. 

Hyoscyamine 
Hydrobromide 
C,7H23N03.HBr. 

Hyoscyamine 
Sulphate 
(C17H23N03)2.H2S04. 

Water                 66.6 

very  soluble 

very  soluble 

Alcohol                 6  .  2 

50 

15.6 

Ether 

0.062 

0.04 

Chloroform          0.133 

40.0 

0.043 

IODINE 
IODINE    I. 


*-  e 

Gms. 

I  per  Liter 

. 

Solution. 

15              O.272-O.283 

25 

0.279 

25 

0.304 

25 

0-339 

25 

0.340 

30 

0-457 

152 


SOLUBILITY  IN  WATER. 


Authority. 

(Dietz  —  Pharm.  Ztg.  43,  290,  '98.) 

(McLauchlan  —  Z.  physik.  Chem.  44,  617,  '03.) 

(Herz  and  Knoch — Z.  anorg.  Chem.  45,  269,  '05.) 

(Jakowkin — Z.  physik.  Chem.  18,  590,  '95.) 

(Noyes  and  Seidensticker  —  Z.  physik.  Chem.  27,  359,  '98.) 

(Dietz.) 


SOLUBILITY  OF  IODINE  IN  AQUEOUS  POTASSIUM  IODIDE 
SOLUTIONS  AT  25°. 

(Noyes  and  Seidensticker;  Bruner  —  Z.  physik.  Chem.  26,  147,  '98.) 


Millimols^per  Liter. 

KI. 

(I2). 

o.ooo 

1.342 

0.830 

1.814 

1.661 

2-235 

3-322 

3-052 

6.643 

4.667 

13.29 

8.003 

26.57 

14.68 

53-15 

28.03 

106.3 

55-28 

Gms.  per  Liter. 


KI. 

I. 

O-OO 

0.340 

i-37 

0.461 

2-75 

0.568 

5'S1 

0-775 

11.03 

1.185 

22  .07 

2.032 

44-I5 

3.728 

88.3 

7.II9 

176.6 

14.04 

Results  by  Bruner. 

Gms.  KI  per  Gms.  I 

1000  g.  Sol.  per  Liter. 

10          0.78* 

20  1. 60 

40  3-25 

60          5  04 

80  6 . 94 

100          8 . 96 


*  There  is  some  uncertainty  in  regard  to  the  position  of  the  decimal  point  in  this  column, 
lation  from  the  original  it  should  be  one  place  further  to  the  right. 


By  caku 


SOLUBILITY  OF  IODINE  IN  AQUEOUS  SALT  SOLUTIONS  AT  25°. 

(McLauchlan.) 

Gms.  Salt  Gms.  Dissolved  I 
per  Liter.        per  Liter. 


Salt. 

Gms.  Salt     Gms.  Dissolved  I 
per  Liter.          per  Liter. 

Na,S04 

29.77 

0.160 

K2SO4 

43-5 

0.238 

(NH4)2S04 

33-o 

0.246 

NaNO3 

85.0 

0.257 

KN03 

IOI  .2 

0.266 

NH4NO3 

8o.O 

o-375 

NaCI 

58-5 

0-575 

KC1 

73-6 

0.658 

Salt. 

NH4C1 

NaBr 

KBr 

NH4Br 

NH4C2H302    77-1 

(NH4)2C2H4    86.9 

H3B03  55.8 


53-4 
103.0 
119.0 

08.0 


o-735 

3-29 

3.801 

4.003 

0.440 

0.980 

0.300 


SOLUBILITY  OF  IODINE  IN  ARSENIC  TRI  CHLORIDE. 

(Sloan  and  Mallet  — Chem.  News,  46,  194,  '82.) 

t°.  o°.  15°.  96°. 

Gms.  I  per  100  gms.  AsCl3        8.42         n.88        36.89 


153  IODINE 

SOLUBILITY   OF   IODINE   IN   AQUEOUS   ETHYL   AND   NORMAL   PROPYL 
ALCOHOL  SOLUTIONS  AT  15°. 

(Bruner  —  Z.  physik.  Chem.  26,  147,  '98.) 

In  Aq.  Ethyl  Alcohol.  In  Aq.  Propyl  Alcohol. 


Gms.           Gms. 

Gms. 

Gms. 

Gms. 

Gms. 

Gms. 

Gms 

C2H6OH        I  per 
per  100  Gms.    100  cc. 
Solvent.      Solution. 

C2H5OH 
per  100  Gms. 
Solvent. 

I  per 

100  CC. 

Sol. 

CaHyOH 
per  loo  Gms. 
Solvent  . 

I  per 

100  CC. 

Sol. 

C3H7OH 
per  loo  Gms. 
Solvent. 

I  per 
loo  cc. 
Sol. 

10        0.05 

60 

I.I4 

10 

0-05 

60 

2.71 

2O           O-o6 

70 

2-33 

20 

O.II 

70 

4-10 

30        o.io 

80 

4.20 

30 

0.40 

80 

6.05 

40           0.26 

90 

7-47 

40 

0.94 

90 

9.17 

50        0.88 

100 

i5-67 

50 

1.64 

100 

M-93 

SOLUBILITY  OF  IODINE  IN  BENZENE,  CHLOROFORM,  AND  IN  ETHER. 

(Arctowski  —  Z.  anorg.  Chem.  n,  276,  '95-'Q6.) 


In  Benzene. 


In  Chloroform. 


In  Ether. 


t°. 

Gms.  I  per  100 
Gms.  Solution. 

A  o             Gms.  I  per  100               .  0 
Gms.  Solution. 

Gms.  I  per  ioo 
Gms.  Solution. 

4-7 

8.08 

-49 

0.188 

-83 

15-39 

6.6 

8.63 

-55i 

0.144 

-90 

14-58 

10.5 

9.60 

-60 

0.129 

-108 

15.09 

13-7 

10-44 

-69i 

0.089 

16.3 

11.23 

-73i 

0.080 

+  10 

i  .  76  pe 

r  ioo  gms.  C 

:HCL 

SOLUBILITY  OF  IODINE  IN  BROMOFORM,  CARBON  TETRA  CHLORIDE,  AND 
IN  CARBON  BISULPHIDE  AT  25°. 

(Jakowkin  —  Z.  physik.  Chem.  18,  590,  '95.) 

i  liter  of  saturated  solution  in  CHBr3  contains  189.55  gms-  I« 
i  liter  of  saturated  solution  in  CC14  contains  30.33  gms.  I. 
i  liter  of  saturated  solution  in  CS2  contains  230.0  gms.  I. 


SOLUBILITY  OF  IODINE  IN  CARBON  BISULPHIDE  SOLUTIONS. 

(Arctowski  —  Z.  anorg.  Chem.  6,  404,  '94.) 


+  o         Gms.  I  per  ioo 
Gms.  Solution. 

t  °. 

Gms.  I  per  ioo 
Gms.  Solution. 

t°. 

Gms.  I  per  ioo 
Gms.  Solution. 

•ioo 

0.32 

o 

7.89 

30 

19.26 

-80 

0.51 

IO 

10.51 

36 

22  .67 

•63 

1  .26 

15 

12-35 

40 

25.22 

-2O 

4.14 

20 

14.62 

42 

26.75 

•10 

5-52 

25 

16.92 

IODINE  154 

SOLUBILITY   OF   IODINE   IN   MIXTURES   OF  CHLOROFORM   AND   ETHYL 

ALCOHOL,  CHLOROFORM  AND  NORMAL  PROPYL  ALCOHOL,  CHLOROFORM 

AND  BENZENE,  AND  CHLOROFORM  AND  CARBON  BISULPHIDE  AT  15°. 

(Bruner.) 


Cms.  CHC13 

Grams  I  Dissolved  per 

A 

ioo  cc.  of  Mixtures  of: 

of  Mixtures.    CHCl3  +  C2H5OH.  CH3C1  +  C3H7OH 

.  CH3C1  +  C6H6. 

CH3C1  +  CS2. 

O 

15.67 

14-93 

IO.4O 

17.63 

IO 

9-43 

13.16 

9.84 

J5-93 

20 

8.69 

ii  .20 

8.78 

14.20 

30 

7.80 

8.98 

7-74 

12.  16 

40 

7.09 

8.09 

6.96 

IO.2O 

50 

6.62     . 

7.82 

6.  20 

Q.OS 

60 

6.24 

7.09 

5-34 

7.72 

70 

5-77 

6.42 

4.89 

6.42 

80 

5  -06 

5-54 

4-53 

S-27 

QO 

4-34 

4-52 

4.07 

4-32 

100 

3.62 

3.62 

3-62 

3  .62 

SOLUBILITY  OF  IODINE  IN  MIXTURES  OF  CARBON  TETRA  CHLORIDE  AND 

BENZENE  AND  IN  MIXTURES  OF  CARBON  TETRA  CHLORIDE 

AND  CARBON  BISULPHIDE  AT  15°. 

(Bruner.) 

Cms.  CCU  per    Cms.  I  per  ioo  cc.  of  Mixture  of:  Gms.  CCUper  Gms.  I  per  ioo  cc.  of  Mixture 

'    CC14  +  CS2.  'SffctSw.     CC14  +  C6H6.  '   CC14+CS2.' 


o  10.40  17.6  60  4.90  5.55 

10  9.44  14-44  7°  4-09  4-50 

20  8.53  12.33  8o  3-4i  3-37 

30  7.77  10.34  90  2.74  2.60 

40  6.63  8.60  ioo  2.06  2.06 

50  5.70  6.83 


SOLUBILITY  OF  IODINE  IN  AQUEOUS  GLYCERINE  SOLUTIONS 

AT   25°. 
(Herz  and  Knoch  —  Z.  anorg.  Chem.  45,  269,  '05.) 

Density  of  glycerine  at  25°/4°  =  I-2555I  impurities  about  1.5% 

Wt.%  Glycerine         Millimols  I  Grams  I  per  Density  of 

inSolvent.      per  ioo  cc.  Solution.      loocc.  Solution.  Solutions  at  25°/ 4°. 

o  0.24  0.0304  Q-9979 

7.15  0.27  0.0342  .0198 

20.44  0-38  o'.o482  -0471 

31.55  0.49,  0.0621  -0750 

40.95  0.69  0.0875  -°995 

48.7  1.07  0.135  .1207 

69.2  2.20  0-278  •I76S 

100.0  9.70  1-223  .2646 


155 


IODINE 


DISTRIBUTION   OF  IODINE    BETWEEN   CARBON   BISULPHIDE    AND 
AQ.  POTASSIUM  OXALATE. 

(Dawson  —  Z.  physik.  Chem.  56,  610,  '06;  Dawson  and  McRae  —  J.  Chem.  Soc.  81,  1086,  '02.) 
Cms.  I  per  Liter  of 


Concentration 

of 
Aq.  K2C204. 

i  .o  Equiv. 

1.0  " 

1.0  " 


Aq.  Layer. 
2.408 

3-555 
5.766 

6.861 


CS2  Layer. 
10.82 
16.32 
27.91 

34-Qi 

17.07 


Vol.  of  Solution 

which  Contains 

i  Mol.  I. 

105-3 

71-37 

43-99 
36.98 
71.97 


Fraction  of  I 
Uncombined 
in  Solution. 

0.005495 


o  005915 
l.o",        6. SOI    34-01         30 .98    0.006055 

1.2  3.525     17.07  71.97     0.005645 

DISTRIBUTION  OF  IODINE  BETWEEN  AMYL  ALCOHOL  AND  WATER  AND 

BETWEEN  AMYL  ALCOHOL  AND  AQUEOUS  POTASSIUM  IODIDE 

SOLUTIONS  AT  25°. 

(Herz  and  Fischer  —  Ber.  37,  4752,  '04.) 

The  original  results  were  plotted  on  cross-section  paper,  and  the 
following  tables  made  from  the  curves. 


Millimols  I  per  10  cc 

JxUlUUKUo  J.    p 

cr  10  uc.  u 

i  n2w  aiiu  oi  /v 

4.  rv.i  x^ayen 

5. 

Amyl  Alcohol  Layer 

'"" 

N 

2N 

jj 

4N 

N      "* 

in  Each  Case. 

HaO. 

—  K.I. 

—  KI 

—  •  K  1  . 

—  KI 

JfT 

10 

10 

10 

10 

IO 

2-5 

0.012 

0-135 

0.160 

O.I7O 

0.170 

3-o 

O.OI4 

0.150 

0.185 

O-2OO 

O.2OO 

0.160 

4-0 

O-Ol8 

0.180 

0-235 

0-255 

0.270 

0.240 

5 

0-021 

O.2IO 

0.280 

o-3J5 

0-340 

0-315 

6 

O.O25 

0.230 

0.330 

0-375 

O.4IO 

0.390 

7 

0.029 

0.250 

o-375 

0.430 

0.480 

0.470 

8 

0.260 

0.420 

0.490 

0-550 

o-555 

9 

0.270 

0.450 

o-55o 

O.62O 

0.640 

10 

O.28o 

0.470 

0.605 

0.690 

0.720 

12 

0.490 

0.700 

0-830 

0.900 

14 

0.510 

0.790 

0.980 

I  .200 

20 

0-575 

Gms.I  per  100  cc. 
Amyl  Alcohol  Layer 

Gms.  I  per 

100  CC.  Of 

H2O  and  of  KI 

Layers. 

N 

N 

N 

N 

N         ^ 

in  Each  Case. 

H20. 

—  K.  I 

•  —  'KL 

—  KI 

—  KI 

KI. 

IO 

IO 

JO 

10 

IO 

3 

O.OI4 

0.164 

O.2O 

O.2I 

O.2I 

4 

0.016 

0.196 

O.24 

O.26 

O.26 

0.21 

6 

0.026 

0.252 

0-34 

0.38 

O.40 

o-37 

8 

0-033 

0.297 

o-43 

0-49 

o-54 

0.51 

10 

0-040 

0.328 

0.51 

0.61 

0.67 

0.69 

12 

0.341 

0-58 

o-73 

0-81 

0.84 

H 

.  .  . 

0.60 

0.83 

o-95 

i  .00 

16 

0.63 

0.91 

1.09 

i  .20 

18 

0.64 

25 

0.71 

The  original  figures  for  sN/io  and  loN/io  KI  solutions  give  prac- 
tically identical  curves. 

Results  for  the  distribution  of  Iodine  between  N/io  KI  solutions  on 
the  one  hand,  and  mixtures  in  various  proportions  of  C6H0+  CS2, 
C6H5CH3+  CS2,  C6H6+  C6H5CH3,  C6H6+  light  petroleum,  CS2  +  light 
petroleum,  CS2+CHC13,  CHC13  +  C6H6,  CC14  +  CS2  and  CC14  +  C6H8CH3 
on  the  other  hand,  are  given  by  Dawson  —  J.  Chem.  Soc.,  81,  1086,  '02. 


IODINE  156 

DISTRIBUTION  OF  IODINE  BETWEEN  WATER  AND  BROMOFORM,  WATER 

AND  CARBON  BISULPHIDE,  AND  WATER  AND  CARBON 

TETRA  CHLORIDE  AT  25°. 

(Jakowkin  —  Z.  physik.  Chem.  18,  590,  '95.) 

Original  results  plotted  on  cross-section  paper  and  table  made  from  curves.  Jakowkin  points  out  that 
the  results  of  Berthelot  and  Jungfleisch  —  Ann.  chini.  phys.  [4]  26,  400,  '72,  are  incorrect  on  account  of 
the  presence  of  HI. 

Grams  I  per  Liter  of  Grams  I  per  Liter  of: 

H20  Layer  in  Each  Case.  CRBr3  £^        CS2  Layer.  CCU  Layer. 

0.0$  20  30  4-0 

o.io          45       60       8-5 
0.15          71       91       J3-0 

0.20  100          126          17.5 

0.25  130          l6o          22.0 

IODOFORM    CHI3,    IODOL   C4I4NH    (Tetra  lodo  Pyrrol). 
SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.  ;  Vulpius  —  Pharm.  Centrh.  34,  117,  '93.) 

«,.       t  *  o  Grams  per  loo^Grams  Solvent. 

CHjjL  CJ4NH. 

Water  25  0.0106                            0.0204 

Alcohol  25  2.14  (1.43  gms.  (V.))  n.i 

Alcohol  b.  pt.  (10.0  gms.  (V.))     .  .  . 

Ether  25  19.2  (16.6  gms.  (V.))  66.6 

Chloroform  25  ...                                 0.95 

IRIDIUM    DOUBLE    SALTS. 

SOLUBILITY  IN  WATER. 

(Palmaer  —  Ber.  23,  3817;  24,  2000,  '91.) 
Double  Salt.  Formula.  f.  Gg^£» 

Irido  Pentamine  Bromide  Ir(NH3)5Br3  12.5             0.284 

Bromonitrate  Ir(NH3)5Br(NO3)2  18                5.58 

"            '*        Trichloride  Ir(NH3)5Cl3  15.1            6.53 

"            "         Chloro  Bromide  Ir(NH3)5ClBr2  15                0.47 

Chloro  Iodide  Ir(NH3)5ClI2  15                0.95 

Chloro  Nitrate  Ir(NH3)5Cl(NO3)2  15.4            1.94 

Chloro  Sulphate  Ir(NH3)5ClSO4.2H2O  15.0            0.74 

Nitrate  Ir(NH3)5(NO3)3  16                0.28 

"    Aquo  Pentamine  Bromide  Ir(NH3)5(OH2)Br3  ord.  temp.  25  .  o 

"          "            Chloride  Ir(NH3)5(OH2)Cl3  ord.  temp.  74.7 

"       "          "            Nitrate  Ir(NH3)5(OH2)(NO3)3  17  10.0 

IRON    BROMIDE    (Ferrous)    FeBr2.6H2O. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  537,  '94.) 


t<>. 

Gms.  FeBr2 
per  100  Gms.  Sol. 

t°. 

Gms.  FeBr2 
per  loo  Gms.  Sol. 

t°. 

Gms.  FeBr2 
per  too  Gms.  Sol. 

—  20 

47-0 

3o 

55-o 

60 

S9-° 

0 

5o-5 

40 

56.2 

80 

6i.S 

20 

53-5 

IOO 

64.0 

IRON    CARBONATE    (Ferrous)    FeCO3. 

100  gms.  H2O  saturated  with  CO2  at  6-8  atmospheres  dissolve  0.073 

gram  FeCO3.  (Wagner  —  Jahresber.  Chem.  135,  '67.) 


157 


IRON    CHLORIDE 


IRON    CHLORIDE 


(Ferrous)    FeCl2.4H2O. 

(Etard.) 


SOLUBILITY   IN  WATER. 


t«. 

Gms.  FeCl2 
per  loo  Gms 
Solution. 

Solid  Phase. 

10 

39-2 

FeCl2.4H20 

15 

40.0 

" 

25 

4i-5 

u 

30 

42.2 

(t 

40 

43-6 

11 

50 

45-2 

u 

60 

80 

87 

90 

IOO 

120 


Gms.  FeCl2 

per  loo  Gms. 

Solution. 

47-o 

50.0 
51.2 

51-4 
51.8 


SoHd  Phase. 

FeCl2.4H2O 

FeCl2.4H20  +  FeCl2 
FeCl2 


SOLUBILITY  OF  IRON  CHLORIDE 

(Roozeboom  —  Z.  physik. 


Mols.Fe2Cl6      Gms-  Feds  per  100 
t°.    per  loo  Mols,  Gms. 

H20.  H20.        Solution. 

Solid  Phase,  Fe2Cl6.i2H2O. 

2-75         49-52      33'12 

2-98      53-6o    34-93 

4-i3       74-39 
91.85 
106.8 
150.0 

201  .7 
23I.I 
246.7 


-55 

-27 

o 

+  20 
30 

37 


42.66 
47.88 
51-64 
60. 01 
66.85 
69.79 
71.15 


5-10 

5-93 
8-33 

30   11.20 
2O   12.83 

8  13-7 

Solid  Phase,  Fe2Cl6.7H2O. 

20     11-35     204.4      67.14 

32   13-55   244.0    70.92 

30  15.12  272.4   73-J3 

25  15.54  280.0  73.69 

Solid  Phase,  Fe2Cl«.5H2O. 
12       12.87       231.8         69.87 
27       14.85       267.5         72.78 


(FERRIC)  Fe2Cl6  IN  WATER. 

Chem.  10,  477,  '92.) 

Mols.  Fe2Cle    Gms-  FeQ3  per  100 
t°.    per  loo  Mols.  Gms. 

HzO.  R20.        Solution. 

Solid  Phase,  Fe2Cl6.sH2O  (con.). 

35  J5-64  281.6  73.79 

50  17-50  3*5-2  75-91 

55  19-iS  344-8  77.52 

55  20.32  365.9  78.54 

Solid  Phase,  Fe2Cl6.4H2O. 

So  19-96  359-3  78-23 

55  20.32  365.9  78.54 

60  20.70  372.8  78.86 

69  21.53  387.7  79.50 
73.5  25.0  450-2  81.81 

70  27.9  502.4  83.41 
66  29.2  525.9  84.03 

Solid  Phase,  Fe2Cl&. 

66  29.2  525.9  84.03 

75  28.42  511.4  83.66 

80  29.20  525.9  84.03 

loo  29.75  535-8  84.26 


SOLUBILITY   OF    FERRIC   CHLORIDE   IN   AQUEOUS   SOLUTIONS   OF 
AMMONIUM  CHLORIDE  AT  25°,  35°,  AND  45°. 

(Mohr  —  Z.  physik.  Chem.  27,  197,  '98.) 

Results  at  25°.     Results  at  35°.     Results  at  45°. 

Solid  Phase 
in  Each  Case. 

Fe2Clfl.i2H20(sB2Oat4S0) 
Hydrate  +  Double  Salt 
Double  Salt 


Double  Salt  +  Mixed  Crystals 
Mixed  Crystals 


NH4C1 


Mols.  per 
loo  Mols.  H2O. 

Mols.  per 
loo  Mols.  H20. 

Mols.  per 
loo  Mols.  H2O. 

NH4C1. 
0 

Fe2Cl6. 
10.98 

NH4C1. 
0 

Fe2Cl.6. 
I3-36 

NH4C1. 

o.o 

Fe2Cl6. 

33-4 

i-S7 

10-74 

1.41 

J3-o5 

2.48 

9-O2 

3.08 

9.28 

4.08 

9-58 

5-28 

7-73 

6.98 

7.64 

9-59 

6-77 

10.76 

6.70 

13.09 

6.31 

9-83 

6.70 

II  .60 

6.52 

13-54 

6.28 

9-65 

6.07 

12.28 

6.08 

12.91 

5-49 

9-93 

5-23 

n-57 

3-98 

J3-49 

4.84 

9.92 

3-97 

11.89 

3-38 

13.46 

4.99 

10.31 

2.05 

13-23 

1  38 

13-30 

0-0 

14.79 

o.o 

16.28 

o.o 

IRON    CHLORIDE 


158 


SOLUBILITY  OF 


Mols.per  TOO  Mols.HgO 


NBUCl. 

Fed*. 

'NH4C1. 

FeCl3. 

o.o 

9-30 

o.o 

83.88 

1.09 

9-57 

3-24 

86.32 

I.36 

9-93 

•4-03 

91  .6l 

2  .OO 

9.27 

5-92 

83.64 

2.79 

8.71 

8.31 

78.77 

4-05 

8.09 

12.08 

73-20 

6.41 

7.18 

19.12 

64-83 

10.78 

6.21 

32.04 

56.00 

7-82 

6-75 

23.21 

60.83 

7.62 

5-94 

22  .63 

53-47 

7.70 

5-03 

22  .90 

45-42 

7.8l 

4-34 

23-23 

39-13 

8-52 

2.82 

25-33 

25-43 

10-95 

0.68 

32-55 

6.15 

11.88 

o.o 

35-30 

o.o 

Solid 
Phase. 


Fe2Cl6.i2H2O 


FERRIC   CHLORIDE    IN  AQUEOUS   SOLUTIONS  OP 
AMMONIUM  CHLORIDE  AT  15°. 

(Roozeboom  —  Z.  physik.  Ch.  10,  148,  '92.) 
Grams  per  TOO  Gms.  H2O . 

Fe2Cl6.i2H2O  -f  Double  Salt 
Double  Salt 


Mixed  Crystals  containing  7.29%  FeCla 
5  -55          " 
4-4  " 

3-8 


0.3I 


NH4C1 


SOLUBILITY  OF  FERRIC  CHLORIDE  IN  AQUEOUS  HYDROCHLORIC  ACID 
SOLUTIONS  AT  DIFFERENT  TEMPERATURES. 

(Roozeboom  and  Schreinemaker  —  Z.  physik.  Chem.  15,  633,  '94;) 


•£ 


,0. 


Gms.  per  100  Gms. 

H20.  Solid 


Mols.  per  100  Mols.    Gms.  per  100  Gms. 

H20.  H20.  Solid 


'  HC1. 

FeCl3. 

HCl. 

FeCl3.    Phase- 

HCl. 

FeCl3. 

HCl. 

FeCl3. 

Phase. 

Results  at  o°. 

Results  at 

25°  (con.). 

O 

8.25 

0 

74- 

3°' 

O 

.0 

29.00 

0.0 

261.!' 

7-52 

6.5I 

15.22 

58- 

62 

7 

•5 

29-75 

15.18 

267.9 

„  Fe2Cle 
cHoO 

13-37 

6-33 

27.06 

57- 

01 

19 

•5 

35-25 

39.46 

3J7-4> 

•5ny^ 

16.80 

8.70 

33-99 

78. 

34 

19 

.5 

35-25 

39.46 

3I7-4l 

18.45 

10.23 

37-34 

92- 

10 

.Fe2Cl6 

20 

.6 

35-34 

41.68 

318.3 

20.40 

15.40 

41.28 

138. 

7 

.i2H2O 

31 

•34 

41.58 

63.42 

374-4 

•  e2.4H2O 

20.10 

16.00 

40.67 

144. 

i 

33 

.00 

43.00 

66.77 

387.3 

19-95 

17.70 

40.37 

159- 

4 

34 

-65 

44.80 

70.11 

403.  4  > 

19.00 
18.05 

22.75 
23.41 

38.45 
36.53 

204. 

2IO. 

8 

8  , 

40 
39 

.41 
-03 

40.  25 
41.38 

81.77 
78.98 

362.4-] 
372.7 

-F^HC, 

18.05 

23.40 

36.53 

210.8    JFeaClfl 

35 

-74 

45-24 

72.33 

407.  4J 

+  4H20 

I9-50 

25-93 

39-55 

233.5    )       -7H2° 

Results  at  40°. 

24.  12 
26.00 
26.00 
34.60 

37-27 
34.60 

30.04 
32.  16 
32.16 
38.11 
36.60 
38.11 

48.81 
52.60 
52.60 
70.01 

75-4i 
70.01 

270. 
289. 
289. 

343- 
329- 
343- 

5 
6 
6 

2 

6 

2 

"*&(> 

F-?3& 

13-4 
13-4 
27.0 

0 

32.4 

37-45 

37-45 
50.80 
58.0 
50.8 

0.0 

27.  II 
27.11 

54.64 

0.0 

291.7 
337-3 
337-3 
457-5. 
522.  3' 

Fc*%> 
**%> 

Results  at  25°. 

42 

.01 

48.64 

85.00 

438-0, 

0.0 
2-33 

10.90 
23-72 

o.o 
4.715 

98. 
213. 

65}FSao 

42 
42 

•50 

.01 

47-52 
48.64 

86.72 
85.00 

fi°rc*Hc> 

438.0)    +4H20 

0.0 

24-5 

0.0 

220 

7  J 

0.0 

23-5 

0.0 

211. 

6] 

Results  for  other  temperatures 

2.33 

23-72 

4.715 

213- 

4    lFe2Cl6 

are 

also   given   in 

the  original 

7-50 

29-75 

15.18 

267. 

9    j       .?H2O 

paper. 

o.o 

3i-5o 

o.o 

283. 

6  } 

159 


IRON    CHLORIDE 


SOLUBILITY  OF  THE  SALT  PAIR  FeCla.NaCl.  IN  WATER  AT  21°. 

(Hinrichsen  and  Sachsel  —  Z.  physik.  Chem.  50,  94,  'o4-'os.) 


Grams  Used. 

Gms.  per  100 
Gms.  Solution. 

G.  Mols.  per 
iooMols.H2O.            Solid 

FeCla.          NaCl. 

FeCl3.              NaCl. 

FeCl3.          NaCl. 

o            3.6 

o            36-10 

O                1  1  .  2      NaCl 

1.8        3.0 

24.27            9.10 

2  .  69           2.8      Mix  Crystals 

3-6        2.5 

25.40            8.45 

2.8l            2.6 

5-5        2.0 

26.40        5  .25 

2-93         2.54 

7-2         1-5 

38-15        3-9o 

4.23            1.22 

9.0         i.o 

45  -38         2.45 

5-03        0.75 

10.8        0.5 

46.75         2.  ii 

5.18        0-65 

10.8        o.o 

83.39        o-o 

9.3              0.0      FeCla 

SOLUBILITY  OF 

THE  SALT  PAIR  FeCla 

,.KC1  IN  WATER  AT  21°. 

(H.  and  S.) 

Grams  Used. 

Gms.  per  100 
Gms.  Solution. 

Gm  .  Mols.  per  100 
Mols.  H20.                      Solid 

FeCl3.       KC1/ 

FeCl3.            KC1.    ' 

-FeCl3.    '       KCi:              PhaSe' 

0          35 

o            34-97 

0                 8.45      KCI 

13          28 

13.44     24.45 

I  .  49         5-9O      Mix  Crystals 

18          21 

23.18      16.54 

2-57      3-99 

23          18.5 

28.05       11-69 

3-II         2.82 

28          16 

35.72       11.68 

3.96         2.82 

3i          10.5 

36-62       11.19 

4  .  06         2  .  70      Double  Salt 

36.2        9 

37-35       13-67 

4-i4      3-3° 

46.5        6 

5^69        7-54 

5.73       1.82 

J5"5        o 

83.89        o.o 

9-3            0.0         FeCl3 

SOLUBILITY  OF 

THE  SALT  PAIR  FeCl3. 

CsCl  IN  WATER  AT  21°. 

(H.  and  S.) 

Grams  Used. 

Gms.  per  100 
Gms.  Solution. 

Gm.  Mols.  per  100 
Mols.  H20.               Solid 

FeC]3.        CsCl. 

FeC]3.          CsCl. 

'Fed,.  '     CsCL 

o          65 

o.o         65.0 

O.O            6.95       CsCl 

O.6         II  .6 

o-45      55  -l8 

°'°5         5-9         FeCls-CsCLHaO 

1-4         10.2 

2.1             52.38 

0.23         5.6 

2.2            8.8 

5.24     51.44 

o-57      5-5 

2.0            7.4 

7.8      47.70 

0.86         5.1         FeCl3.2CsCl.H2O 

3.8        6.0 

8.93     41.15 

0.99      4.4 

4-6         4.6 

J5-34       25.25 

1.70     2.7 

5-4        2.8 

21.65     14.96 

2  .  40      1.6 

6.2         1.4 

27.96        8.42 

3.10      0.9 

35-0            0.2 

48.71        0-94 

5-40      o.i 

35.0        o.o 

83.89        o.o 

9.3        o.o      FeCi3 

100  gms.  abs.  acetone  dissolve  62.9  gms.  FeCl3  at  18°. 

(Naumann  — Ber.37,  4332,  '04.) 


IRON    NITRATE  160 

IRON    NITRATE    (Ferrous)    Fe(NO3)5 


Solid 
Phase. 

-27  35-66         5.54      Fe(N03)2.9H20  ~9  39-68         6.57     Fe(NO3)2.6H2O 

-21-5 

-15-5 

Density  of  solution  saturated  at  18°  =  1.497. 

IRON    OXIDES,    HYDROXIDE    and    SULPHIDE. 

SOLUBILITY  IN  AQUEOUS  SUGAR  SOLUTIONS. 

(Stolle  —  Z.  Ver  Zuckerind.  50,  340,  'oo.) 


SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  438,  'oo.) 

Cms. 

Mols. 

Gms. 

Mols. 

Fe(NO3)2 

Fe(N03)2            S()lid 

Fe(N03)2 

Fe(N03)2 

per  loo 
Gms. 

^rois~       «-• 

t  °. 

per  100 
Gms. 

per  100 
Mols. 

Sol. 

H2O. 

Sol. 

H20. 

35-66 

5  •  54      Fe(N03)2.9H20 

-9 

39.68 

6-57 

36.10 

5  •  64 

0 

41  .53 

7-10 

36-56 

5.76 

18 

45-14 

37-17 

5.91 

24 

46.51 

8.70 

60.5 

62.50 

16.67 

70  Sugar                                   One  Liter  of  Sugar  Solutions  Dissolves  Milligrams  of: 
in  Sol-           Fe2(OH)6at:                     Fe2O3  at:                             Fe3O4  at: 

FeS  at: 

vent. 

17-4°. 

45°  • 

75°. 

17-5°. 

45°. 

17-5°. 

45°- 

75°. 

17-5°. 

45°. 

75°.  ' 

10 

3-4 

3-4 

6.1 

1.4 

2  .O 

10-3 

10-3 

12-4 

3-8 

3-8 

5-3 

30 

2-3 

2.7 

3-8 

1.4 

12-4 

10-3 

12-4 

7-i 

9.1 

7-2 

50 

2-3 

1.9 

3-4 

0.8 

I.I 

14-5 

10-3 

14-5 

9-9 

19.8 

9.1 

IRON    PHOSPHATE    Fe2(PO4)3. 

THE  ACTION   OF  WATER  AND   OF  AQUEOUS   SALT  SOLUTIONS   UPON 
FERRIC  PHOSPHATE. 

(Lachowicz  —  Monatsh.  Chem.  13,  357,  '92;  Cameron  and  Hurst  —  J.  Am.  Chem.  Soc.  26,  888,  '04.) 

The  experiments  show  that  the  ordinary  precipitation  methods  for 
the  production  of  ferric  phosphate  give  products  which  do  not  conform 
to  the  formula  Fe2(PO4)3.  By  digesting  such  samples  with  water 
very  little  is  dissolved,  but  the  material  is  decomposed  to  an  extent 
depending  upon  the  relative  amounts  of  solid  and  solvent  used.  The 
amount  of  PO4  dissolved  per  gram  of  Fe2(PO4)3  varies  from  about 
0.0026  gram  removed  by  5  cc.  H2O  to  0.0182  gram  removed  by  800  cc. 
H2O  at  the  ordinary  temperature. 

IRON    SULPHATE    (Ferrous)    FeSO4.7H2O. 
SOLUBILITY  IN  WATER. 

(Franckel  —  Heidelberg  '05,  Landolt  and  Bernstein's  Tabellen,  3d  ed.  p.  537,  '06.) 

Cms.  FeSO4  -,..  Cms.  FeSO4                  «,,.. 

t°.                 per  100  £?lld  t°.             per  TOO                        £°lld 

Gms.H20.  Phase"  Gms.H20.                   Phase' 

—  I  .  82            14  . 98  Ice+FeSO4.7H2O  56.6            54 . 58    FeSO4-7H2O  -f-  FeSO4.4H2O 

O                    I5-62  FeSO4-7H2O  60                 55 -°2                 FeSO4-4H2O 

10  20.85  "  70  56.04 

20  26.42  «  75.8  56.8      FeS04.4H20  +  FeS04.H20 

30  33-00  "  80  50.6  FeS04.H2O 

40  40.20  »  90  43.0 

50  48.55 

ioo  grams  sat.  solution  in  Glycol  contain  6.0  grams  FeSO4  at  ordi- 
nary temperature.  (de  Coninck.) 


161     IRON  POTASSIUM  SULPHATE 


IRON  POTASSIUM  SULPHATE  (Ferrous)  FeSO4.K2SO4.6H2O. 
SOLUBILITY  IN  WATER. 

(Tobler  —  Liebig's  Ann.  95,  193,  '55.) 


t°. 

Cms.  K2Fe(S04)2 
per  100  Grams 
H20. 

o 

19.6 

10 

24-5 

14.5 

16 
25 

29.1 
30-9 
36.5 

t°. 

Cms.  K2Fe(S04)2 
per  loo  Grams 

H-jO. 

35 

41-0 

40 

45  -o 

55 

56.0 

65 

57-3 

70 

64.2 

SOLUBILITY  OF  MIXTURES  OF   FERROUS   SULPHATE   FeSO4.7H2O   AND 
SODIUM  SULPHATE  Na2SO4.ioH2O  IN  WATER. 

(Koppel  —  Z.  physik.  Chem.  52,  405,  '05.) 


Gms.  per  100  Gms. 
t°.                     Solution. 

Gms.  per  TOO  Gms. 
H20. 

FeS04. 

Na2SO4. 

FeSO4. 

Na2SO4. 

O 

14. 

54 

4-93 

18 

.06 

6 

.11 

15-5 

i7- 

76 

ii 

•32 

25 

•05 

I5 

•97 

21.8 

16. 

57 

15 

•32 

24 

•34 

22 

•51 

24.92 

16. 

21 

15 

•13 

23 

.62 

22 

.04 

35 

16. 

35 

14 

.98 

23 

.91 

21 

•83 

40 

16. 

37 

15 

.42 

24 

.01 

22 

.62 

18.8 

18. 

13 

.8 

26 

•63 

20 

.28 

23 

19. 

58 

12 

•5 

28 

.82 

18 

•4 

27 

20. 

97 

II 

•3 

30 

•95 

16 

.64 

31 

22  . 

91 

9 

.71 

33 

•99 

14 

.41 

35 

23- 

85 

9 

.26 

35 

.61 

13 

•85 

40 

26. 

32 

7 

•85 

39 

.98 

II 

.92 

18.8 

18. 

23 

14 

•83 

27 

•23 

22 

.16 

23 

13  . 

83 

18 

.04 

20 

.31 

26 

.48 

28 

7- 

66 

24 

.41 

ii 

.28 

35 

•94 

31 

4- 

58 

29 

•5° 

6 

•95 

44 

•75 

35 

4- 

04 

30 

•49 

6 

.16 

46 

-58 

40 

4- 

10 

30 

.60 

6 

•27 

46 

99 

Solid  Phase. 


FeSO4.7H2O  +  Na2SO4.ioH2O 


FeNa2(S04)2.4H20 


FeNa2(SO4)2.4H20  +  FeSO4.7H2O 


FeNa2(SO4)2.4H2O  +  Na2SO4.ioH2O 


FeNa2SO44H20  +  NaaSO4 


(Marignac.) 


LANTHANUM    BROMATE  162 

LANTHANUM    BROMATE    La(BrO3)3.9H2O. 

100  gms.  H2O  dissolve  28.5  gms.  lanthanum  bromate  at  15°. 

LANTHANUM    SULPHATE    La2(SO4)3. 

SOLUBILITY  IN  WATER. 

(Muthmann  and  Rolig —  Ber.  31,  1723,  '98.) 

0      Gms.  La2(SO4^3  per  100  Gms.  0      Gms.La2(SO4)3per  looGi 

Solution.        Water.'  Solution.        Water.' 

o          2.91         3.0  50          1.47         1.5 

14          2.53        2.6  75          0.95        0.96 

30          1.86         1.9  100          0.68        0.69 

LEAD    Pb. 

MUTUAL  SOLUBILITY  OF  LEAD  AND  ZINC. 

(Spring  and  Romanoff  —  Z.  anorg.  Chem.  13,  34,  '96.) 
Upper  Layer.  Lower  JLayer.  Upper  Layer.  Lower  Layer. 


•2-J/1 

%pb. 
98  8 

%Zn. 
I    2 

%pb. 

C7 

Zn. 

6^0 

%p 
82 

b.      %Z 

OT*7 

n. 

7f) 

%Zn/ 

GOT" 

419 

Q2  -O 

8.0 

i-5 

98 

•5 

740 
800 

°6  • 
79- 

*7 

0       21 
O       2  C 

•  O 

Q 

.0 
IO-O 

14  o 

93  -° 
90.0 
86  o 

475 
584 

91  .0 
86.0 

9.0 
14.0 

2.0 

5-o 

98 

95 

•  O 

.0 

900 

910-920 

59- 
(crit. 

u      ^5 
o     41 
temp. 

.0 

) 

25-5 

74-5 

LEAD    ACETATE    Pb(C2H3O2)2.3H2O. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 


Solvent. 


(U.  S.  P.) 
Grams  Pb(C2H3O2)2  per  100  Grams  Solvent  at: 


25°.  b.  pt. 

Water  50                                              200 

Alcohol  3.3                                            ioo 

Alcohol  (0.941  Sp.  Gr.)  12.5  (per  ioo  cc.  at  15  .5°) 

Glycerine  20.0  (15°) 


LEAD    BENZOATE    Pb(C7H6O2)2.H2O. 

SOLUBILITY  IN  WATER. 

(Paietta  —  Gazz.  chim.  ital.  36,  II,  67,  '06.) 
t°.  18°.  40.6°.  49.5°. 

Gms.  Pb(C7H5O2)2.H2O 
per  ioo  gms.  sat.  solution          0.149        0.249        0.310 


LEAD    BROMATE    Pb(BrO3)2.H2O. 

ioo  gms.  cold  water  dissolve  1.33  gms.  lead  bromate. 

(Rammelsberg  —  Pogg.  Annalen.  52,  96,  '41;  Bottger  — Z.  physik.  Chem.  46,  602,  '03.) 


LEAD    BROMIDE 


163 
PbBr2. 

SOLUBILITY  IN  WATER. 

(Lichty  —  J.  Am.  Chem.  Soc.  25,  474,  '03.) 


LEAD    BROMIDE 


Density 
t°            of  Solutions 

Gms.  PbBr2  per  100 

Milligram  Mols.  PbBf2  per  too 

H2O  at  o°.' 

cc.  Solution. 

Gms.  H2O. 

cc.  Solution. 

Gms.  H2O. 

o         1-0043 

Q-4554 

0-4554 

I  .242 

I  .242 

15 

•0053 

0.7285 

•0.7305 

1.987 

1.989 

25 

.0061 

0.9701 

0-9744 

2  .646 

2-655 

35        ^ 

.0060 

1.3124 

i  .3220 

3-577 

3-603 

45 

.0059 

J-7259 

I-7457 

4-705 

4-760 

55 

.0046 

2  .IO24 

2.1376 

5-73i 

5-827 

65 

.0028 

2.516 

2-574 

6.859 

7.0l6 

80 

.0000 

3-235 

3-343 

8.819 

9-II3 

95        0.9995 

4.1767 

4-3613 

11.386 

I  I  .  890 

IOO 

4-550 

4-751 

12.40 

12.94 

SOLUBILITY  OF  LEAD  BROMIDE  IN  AQUEOUS  HYDROBROMIC  ACID 

AT    10°. 

loo  grams  H2O   containing   72.0   grams  HBr  dissolve   55.0  grams 
PbBr2  per  100  gms.  solvent,  and  solution  has  Sp.  Gr.  2.06. 

(Ditte  —  Compt.  rend.  92,  719,  '81.) 

LEAD    CARBONATE    PbCO3. 

SOLUBILITY  IN  WATER  BY  ELECTRICAL  CONDUCTIVITY  METHOD. 

(Kohlrausch  and  Rose  —  Z.  physik.  Chem.  12,  241,  '93;  Bottger  —  Ibid.  46,  602,  '03.) 

i  liter  of  water  dissolves  o.oon   —  0.0017  gram  PbCO3  at  20°. 

LEAD  CHLORATE  Pb(ClO3)2. 

loo  grams  H2O  dissolve  151.3  grams  Pb(ClO3)2,  or  100  grams  sat. 
solution  contain  60.2  gms.  Pb(ClO3)2  at  18°.     Density  of  solution,  1.947. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 


LEAD    CHLORIDE    PbCl2. 

SOLUBILITY  IN  WATER. 

(Lichty;  see  also  Formanek  —  Chem.  Centrb.  18,  270,  '87;  Bell  —  Chem.  News,  16,  69,  '67;  Ditte 
Compt.  rend.  92,  718,  '81.) 


t°. 

Density 

Gms.  PbCl2  per  100 

Milligram  Mols^.  PbCl2  per  TOO 

°H20  a/  o°!' 

cc.  Solution. 

Gms.  H2O, 

cc.  Solution. 

Grams  H2O. 

0 

I  .0066 

0.6728 

0.6728 

2  .421 

2  .421 

J5 

I  .  0069 

0.9070 

o  .  9090 

3-265 

3.272 

25 

I  .0072 

1.0786 

I  .0842 

3.882 

3-903 

35 

I  •  0060 

I-3I50 

1.3244 

4-733 

4.767 

45 

I  .  OO42 

1.5498 

!-5673 

5-579 

5-644 

55 

I  .  OO2O 

I  .8019 

1.8263 

6.486 

6-573 

65 

0.9993 

2-o8lO 

2  .1265 

7.490 

7-651 

80 

0-9947 

2.5420 

2  .6224 

9.150 

9-439 

95 

0.9894 

3-0358 

3-I654 

10.926 

n-394 

IOO 

3.208 

3-342 

11.52 

12  -OI 

LEAD    CHLORIDE 


164 


SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC ACID. 


(At  o°,  Engel  —  Ann.  chim.  phys.  [6]  17,  359,  '89;  at  25°,  Noyes  —  Z.  physik.  Chem.  9,  623, 
ent  temperatures,  Ditte  —  Compt.  rend.  92,  718,  '81;  see  also  Bell  —  J.  Chem.  Soc.  21, 

'92;  at  differ- 
350,  '68.) 

Gms.  HCl        Gms.  PbCl2  per 

per  loo 

Gms.  PbCl2  per  100  Gms.  Solution  at: 

Liter. 

0°. 

25°. 

Gms.  H20. 

0°. 

20°.                 40°. 

55°. 

'    80°. 

O 

5 

•83 

IO 

•79 

O 

8 

•  O 

ii.  8     17.0 

21  . 

0 

3I.O 

O-5 

4 

•5 

9 

.0 

IOO 

i 

.2 

i-4      3-2 

5 

•5. 

12.0 

1.0 

3 

.6 

7 

.6 

150 

i 

•5 

2  .0      5  .0 

7' 

q 

16.0 

2-O 

2 

.2 

6 

.0 

200 

3 

•5 

5.0      8.2 

ii  . 

fj 

21.5 

3-0 

I 

.6 

5 

•  o 

250 

6 

•5 

8.0     13.0 

16, 

2 

28.5 

6 

I 

•4 

3 

.1 

300 

10 

•7 

12-5     I7-S 

22. 

O 

35-o 

10 

I 

.2 

i 

.8 

4OO 

21 

•5 

24.0 

. 

IOO 

I 

.2 

. 

2OO 

5 

.2 

. 

250 

IO 

•5 

. 

300 

17 

•5 

. 

400 

40 

.0 

•. 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  AQUEOUS  SALT  SOLUTIONS 

AT  25°. 

(Noyes;  in  HgQ2  solutions  at  20°,  Formanek  —  Chem.  Centralb.  270,  '87.) 

In  Aqueous  Solutions  of: 


HCl,  KC1,  MgCl2,  CaCl2,  MnCl2         In  CaCl2 
and  ZnCl2  Gram  Equivalents         Gram  Equiv. 
per  Liter  of:                         per  Liter. 

In  HgCl2 
Gram  Equiv. 
per  Liter. 

In  Pb(N03)2 
Gram  Equiv. 
per  Liter. 

'Salt.           PbCl2.               CdCl2.        PbCl2. 

o.o      0.0777        °-°°    0.0777 
0.05     0.050          0.05     0.0601 
o.io    0.035          o.io    0.0481 

O.2O      O-O2I               O-2O      O.O355 

HgCl2.      PbCl2. 

o.o    0.0777 
o.i     0.0992 

Pb(N03)2.        PbCl2. 

o.o        0.0777 

O.2            0.0832 

The  above  results  were  calculated  to  grams  per  liter  plotted  on  cross- 
section  paper,  and  the  figures  in  the  following  table  read  from  the 
curves. 


Gms.  Salt 


Grams  PbCl2  per  Liter  in  Aqueous  Solutions  of: 


per 
Jter, 

HCl. 

KC1. 

MgCl2. 

CaCl2. 

MnCl2. 

ZnCl2.       CdCl2. 

HgCl2. 

Pb(N03)2 

O 

10.79 

10.79 

10.79 

10.79 

10.79 

10.79     10 

•79 

io.79( 

N)  9 

•7i(F) 

10.79 

I 

8-5 

9-3 

7-7 

8.7 

9-5 

IO 

.2 

ii  .0 

9 

.8 

10.8 

2 

6-5 

8.2 

6-5 

7.6 

8-3 

9 

•7 

11.4 

IO 

.0 

10.85 

3 

S-2 

7-2 

5-7 

6.7 

7-3 

9 

.2 

11.7 

IO 

•3 

10.87 

4 

4-3 

6.5 

5-2 

6.0 

6-3 

8 

.6 

12.0 

10 

•5 

10.90 

6 

3-2 

5-3 

4.4 

4.8 

5-o 

7 

•7 

12.7 

II 

o 

10.95 

8 

2-5 

4-5 

3-9 

4.1 

7 

.0 

13-3 

II, 

6 

ii  .00 

IO 

2.  I 

3-9 

3-3 

3-5 

6 

•3 

14.0 

12. 

2 

ii  .05 

14 

.  .  . 

3-1 

.  .  . 

.  .  . 

2.8 

3-o        5 

•4 

.  .  . 

*3  • 

2 

11.15 

20 

T  A 

8 

ii  .  20 

40 

10 

,0 

11.70 

165  LEAD    CHLORIDE 

SOLUBILITY  OF  LEAD  CHLORIDE  IN  GLYCERINE. 

(Presse  —  Ber.  7,  599,  '74.) 

i  part  glycerine  +  7  parts  H2O  dissolve  0.91  per  cent  PbCl2. 
i  part  glycerine  +  3  parts  H2O  dissolve  1.04  per  cent  PbCl2. 
i  part  glycerine  +  i  part  H2O  dissolves  1.32  per  cent  PbCl2. 
Pure  glycerine  dissolves  2.00  per  cent  PbCl2. 

LEAD    CHROMATE    PbCrO4. 

One  liter  of  water  dissolves  0.0002  gram  PbCrO4  at  18°  (conductivity 

method).  (Kohlrausch  — Z.  physik.  Chem.  50,  365,  'o4-'os.) 

SOLUBILITY  OF  LEAD  CHROMATE  IN  AQUEOUS  POTASSIUM  HYDROXIDE 

SOLUTIONS. 

(Lacland  and  Lepierre  —  Bull.  soc.  chim.  [3]  6,  230,  '91.) 

t  °.  Grams  KOH  per  100  cc.    Grams  PbCrO4  per  100  cc. 

15  2.308  I.I9 

60  2.308  1.62 

80  2.308  2.61 

102  2.308  3.85 

LEAD    CITRATE    Pb(C6H5O7)2.H2O. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

100  gins.  H2O  dissolve  0.04201  gm.  Pb(C6H5O7)2.H2O   at   18°,  and 
0.05344  gm.  at  25°. 

100  gms.  alcohol  (95%)  dissolve  0.0156   gm.  Pb(C6H6O7)2.H2O   at 

l8°,  and  0.0167  gm-  at  25°-  (Partheil  and  Hubner  —  Archiv.  Pharm.  241,  413,  '03.) 

LEAD    DOUBLE    CYANIDES. 

SOLUBILITY  IN  WATER. 

(Schuler  —  Sitzber.  Akad.  Wiss.  Wien,  79,  302,  '79.) 
Double  Salt.  Formula.  t°.    G^S^2Q°° 

Lead  Cobalticyanide  Pbg[Co(CN)6]2.7H2O  18  56. 5*' 

Lead  Cobalticyanide  PbJCo(CN)6]2.7H2O  19  61.3 

Lead  Potassium  Cobalticyanide  PbKCo(CN)6.3H2O  18  14.8 

Lead  Cobalticyanide  Nitrate       Pb3[Co(CN)6]2.Pb(NO3)2.i2H2O  18          5.9 
Lead  Ferricyanide  Nitrate  PblFe(CN)6]2.Pb(NO3)2.i2H2O   16          7.5 

Lead  Potassium  Ferricyanide      PbKFe(CN)6.3H2O  16  21.0 

LEAD    FLUORIDE    PbF2. 

One  liter  of  water  dissolves  0.64  gram  PbF2   at    18°  (conductivity 

method) .  (Kohlrausch  —  Z.  physik.  Chem.  50,  365,  'o4-'o5.) 

LEAD    FORMATE    Pb(HCOO)2. 

SOLUBILITY  OF  LEAD  FORMATE  IN  AQUEOUS  SOLUTIONS  OF  BARIUM 

FORMATE  AT  25°. 

(Fock  — Z.  Kryst.  Min.  28,  383,  "97-) 


Mol.  %  in  Solution. 

Grams  per  Liter.                 gp.  Gr.  of 

In  Solid  Phase  Mol.%  of 

Pb(HC02)2. 

Ba(HC02)2'. 

Pb(HC02)2. 

Ba(HCO2)2.     Solutions. 

Pb(HC02)2. 

Ba(HC02)2. 

o.oo 

100.  0 

28.54 

.2204 

0-0 

100 

0.29 

99.71 

I.I04 

28.65 

.2213 

1.72 

98.28 

0-74 

99.26 

2.803 

28.90 

.2251 

5'29 

94.71 

1.24 

98.76 

5-309 

32.24 

.2529 

11-94 

88.06 

2.91 

97.09 

II  .42 

29.29 

.2341 

24.81 

75  -J9 

5-92 

94.08 

23.11 

28.13            1.2355 

56.54 

43-46 

100.00 

o.o 

28.35 

I.09II 

100.  0 

0-0 

LEAD    HYDROXIDE 


166 


LEAD    HYDROXIDE    Pb(OH)2. 

SOLUBILITY  OF  LEAD  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
HYDROXIDE.     (Moist  Lead  Hydroxide  used,  temperature  not  given.) 

(Rubenbauer  —  Z.  anorg.  Chem.  30,  336,  '02.) 

Grams  per  100  cc.  Solution. 


Amt.  of  Na 
in  20  cc. 

Amt.  of  Pb. 
in  20  cc. 

Mol.  Dilution 
of  NaOH. 

O.2O24 

O-IOI2 

2  .27 

0-3196 

0.1736 

1.44 

0.5866 

0-3532 

0-785 

0.9476 

0.4071 

0.485 

1.7802 

0.5170- 

0.258 

NaOH. 

i-759 
2.778 
5.10 
8-235 
I5-470 


Pb(OH)2. 
0.590 
I  -OIO 
2.056 
2.370 

3-Qio 


LEAD    IODATE    Pb(IO3)2. 
One  liter  of  water  dissolves  0.019  gm.  Pb(IO3)2  at  18°. 


(Kohlrausch;  Bottgero 


LEAD    IODIDE    PbI2. 


SOLUBILITY  IN  WATER. 

(Lichty  — J.  Am.  Chem.  Soc.  25,  471,  '03.) 


t°. 

Density. 

Grams  PbI2  per  100 

Millimols  PbI2  per  100 

(H2O  at'o°.) 

cc.  Solution. 

Grams  H2O. 

cc.  Solution. 

Grams  H2O. 

o 

I  .  OOO6 

O.O442 

o  .  0442 

0-096 

0-096 

J5 

o  .  9998 

0-0613 

0.0613 

0-133 

0-133 

25 

o  .  9980 

0-0762 

0.0764 

0.165 

0.166 

35 

0.9951 

0-1035 

o  .  1042 

0.224 

0.226 

45 

0.9915 

o  .  1440 

0-1453 

0.312 

0-3*5 

55 

0.9872 

0.1726 

0-1755 

o-374 

0.381 

65 

0.9827 

O.2I4O 

0.2183 

0.464 

o-473 

80 

0-9745 

0-2937 

0.3023 

0.637 

0.656 

95 

0.9671 

0-3814 

0.3960 

0.828 

0.859 

100 

O.42O 

0.436 

0.895 

0.927 

SOLUBILITY  OF  LEAD  IODIDE  IN  ACETONE,  ANILIN  AND  AMYL  ALCOHOL. 

(von  Laszczynski  —  Ber.  27,  2285,  '94.) 

Grams  PbI2  per  100  Grams  Solvent. 
O.02 
0.50 


Solvent. 

(CH3)2CO 
C6H5NH2 
C6H5NH2 
C5H7OH 


t° 

59 

13 

184 


i  .10 

0.02 


i67 


LEAD    IODIDE 


SOLUBILITY  OF  MIXTURES  OF  LEAD  IODIDE  AND  POTASSIUM  IODIDE 

IN  WATER. 

(Ditte  —  Ann.  chim.  phys.  [5]  24,  226,  '81;  Schreinemaker  —  Z.  physik.  Chem.  9,  65,  '92.) 


•/     . 

PbI2. 

KI. 

Pbi2. 

K2I2. 

Phase. 

5 

I63 

8.8 

Double  Salt  +  PbI2 

2O 

9 

260 

o-3 

14.1 

.. 

28 

25 

325 

0.9 

17.6 

.. 

39 

45 

449 

1.8 

24-3 

" 

67 

255 

751 

9-9 

40.7 

««                 i> 

80 

731 

1186 

28.5 

64-3 

« 

80 

519.9 

976.4 

22  .2 

52-9 

4.                                  It 

104.5 

1411 

1521 

55  .1 

82.5 

.« 

120 

2151 

1812 

83-9 

98.2 

" 

137 

2874 

2097 

112  .2 

113.8 

.1 

175 

5603 

2947 

218.7 

159-9 

« 

189 

3339 

181.0 

I. 

9 

96.6 

1352 

3-77 

73-3 

Double  Salt  +  KI 

13 

114.3 

1384 

4.46 

75-05 

„ 

23 

186.3 

1510 

7.27 

81.08 

"                 " 

5o 

526.7 

1906 

20.56 

103-3 

it                 it 

64 

789.3 

2161 

30.8 

117.2 

ti                 i. 

83-5 

1108.6 

2434 

43-2 

I3I-9 

it                 u 

92 

1273 

2566 

49-7 

139-3 

u 

137 

2382 

3278 

93-o 

117.7 

" 

165 

4187 

4227 

163.4 

229.1 

«, 

218 

10303 

402.3 

.  .  . 

u 

241 

12803 

7998 

499-9 

433  -6 

t, 

242 

12749 

497-8 

„                        .< 

250 

15264 

596.0 

I, 

t°. 

Gms.  PbI2.2KI  per 
1000  Gms.  H2O. 

Mols.  PbI2.2KI  per 
1000  Mols.  H2O. 

157 

5218 

141.07 

172 

6489 

I7S-S 

186 

7903 

213-7 

194 

9266 

250.6 

2OI 

II320 

306.0 

Solid  Phase. 
PbI2.2KI.2}H,O 


LEAD    MALATE    Pb.C4H4O5.3H2O. 

SOLUBILITY  IN  WATER  AND  ALCOHOL. 

(Partheil  and  Hiibner —  Archiv.  Pharm.  241,  413,  '03.) 

ioo   gms.    H2O    dissolve   0.0288   gm.    PbC4H4O5.3H2O   at    18°,    and 
0.06504  gm.  at  25°. 

ioo  gms.  95%  alcohol  dissolve  0.0048  gm.  PbC4H4O6.3H2O  at  18°- 


25°- 


Density  of  alcohol  employed  =  0.8092. 


LEAD    NITRATE  168 

LEAD    NITRATE    Pb(NO3)2. 

SOLUBILITY  IN  WATER. 


(Mulder; 

Kremers  —  Pogg.  Ann.  92,  497,  '54;  at  15°,  Michel  and  Kraft  —  Ann.  chim 
471,  '54;  at  17°,  Euler  —  Z.  physik.  Chem.  49,  314,  '04.) 

Grams  Pb(NOg)2  per  100  Gms.                   i0            Grams  Pb(NO3)2  per 

.Phys.  [3], 
TOO  Gms. 

*    '            '        Water. 

Solution. 

27-33 
31.6 

34-2 
35-2 

36-9 
38.8 

* 

(3) 
Euler 

40 

SO 
60 
80 
IOO 

17° 

Water. 

Solution. 
41-9 

45-o 
47.8 

52-7 
34-54" 

O 

10 

17 

20 

25 
30 

36 
44 

So 
52 
56 
60 

•4 

.0 

•3 
•4 

•7 

:»    38 
48 
54 
56 
60 
66 

.8<2) 
•3 

.0 

•5 
.6 
.0 

69 

78 

88 
107 
127 
52 

•4        75 
•7        85 
•o        95 
.6      115 
o      138 
,76* 

.0 
.0 
.0 
.0 
.8 

(i)  Mulder,  (2)  Kremers,  (3)  Average  of  M  and  K. 
Density  of  saturated  solution  at  17°  =  1.405.     (Euler.) 

SOLUBILITY  OF  LEAD  NITRATE  IN  ETHYL  AND  METHYL  ALCOHOL. 

Gms.  Pb(NO3)2  per  100  Grams  Solvent  at: 
Solvent.  , ^ p 

Aq.  C2H5OH  (Sp.  Gr.  .9282)    4.96    5.82    8*77  xs.8    14*9    (G) 

Abs.  C2H5OH  o. 04  (20.5°)      (de  B) 

Abs.  CH3OH  1.37    " 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  129,  '65;  de  Bruyn  —  Z.  physik.  Chem.  10,  783,  'p2-) 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  LEAD  NITRATE  AND  STRONTIUM 


NITRATE  IN  WATER  AT  25°. 

(Fock  —  Z.  Kryst.  Min.  28,  372,  '97.) 

Mol.  per  cent  in  Solution. 

Gms.  per  100  cc.  Solution. 

Sp.  Gr.  of 

Mol.  per  cent  in  Solid  Phase. 

Pb(N03)2. 

Sr(N03)2. 

Pb(N03)2. 

Sr(N03)2. 

Solutions. 

Pb(N03)2. 

Sr(N03)2. 

IOO 

O 

.0 

46.31 

o.o 

I 

•4472 

IOO 

O 

.0 

87 

.41 

12 

•39 

50-47 

4-56 

I 

•4336 

99 

•05 

O 

•95 

78 

.68 

21 

•32 

53-92 

8.14 

I 

.4288 

98 

.11 

I 

.89 

56 

•39 

43 

.61 

45-34 

17.81 

I 

.4263 

97 

.02 

2 

.98 

60 

.29 

39 

•7i 

44.48 

18.74 

I 

•4245 

96 

.06 

3 

•94 

33 

.70 

66 

•30 

25-23 

35-03 

I 

.4468 

83 

.84 

16 

.16 

24 

•58 

75 

.42 

I9-I3 

37-54 

I 

.4867 

32 

.88 

67 

.12 

o 

•  o 

IOO 

•  o 

o.o 

71.04 

I 

•SMi 

0 

.0 

IOO 

.00 

LEAD    OXALATE    PbC2O4. 

One  liter  of  water  dissolves  0.0015  gm-  PbC2O4  at  18°  (conductivity 

method).  (Bottger  — Z. physik.  Chem.  46,  602,  '03;  Kohlrausch  —  Ibid  50,  356,  'o4-'os.> 

LEAD    OXIDES.  SOLUBILITY  IN  WATER. 

(Bottger;  Ruer  —  Z.  anorg.  Chem.  50,  273,  '06.) 
No.  Description  of  Oxide.  ^rfltt'     pe?Lher. 

1.  Yellow  Oxide,  by  boiling  Pb  hydroxide  with  10%  NaOH  i .  03  X  io~4  o.  023 

2.  Red  Oxide,  by  boiling  Pb  hydroxide  with  cone.  NaOH  0.56X10"*  0.012 

3.  Yellow  Oxide,  by  heating  No.  i  to  630°  1.05X10"*  0.023 

4.  Yellow  Oxide,  by  heating  No.  2  to  740°  i.ooXio"4  0.022 

5.  Yellow  Oxide,  by  heating  com.  yellow  brown  oxide  to  620°  i .  09  X  io~4  o.  024 

6.  Yellow  Brown  Oxide  commercially  pure  1.10X10"*  0.024 

7.  Yellow  Brown  Oxide,  by  long  rubbing  of  No.  5.  1.12X10"*  0.025 

Bottger  gives  for  three  samples  of  lead  oxide,  0.017,  0.021,  and  0.013 
gm.  per  liter  respectively. 


i6(>          LEAD  PALMITATE 

LEAD  PALMITATE,  LEAD  STEARATE. 

100  cc.  absolute  ether  dissolve  0.0138  gm.  palmitate  and  0.0148 
gm.  stearate. 

(Lidoff  —  Bull.  soc.  chim.  [3]  10,  356,  '93.) 

LEAD    PHOSPHATE    (Ortho)    Pb3(PO4)2. 

One  liter  of  4.97  per  cent  aqueous  acetic  acid  solution  dissolves  1.27 
gms.  Pb3(P04)2. 

(Bertrand  —  Monit.  Scient.  [3]  10,  477,  '68.) 

LEAD    SUCCINATE    PbC4H4O4. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Partheil  and  Hubner  —  Archiv.  Pharm.  241,  413,  '03.) 

ioo  gms.  H2O  dissolve  0.0253  gm-  PbC4H4O4  at  18°,  and  0.0285 
gm.  at  25°. 

ioo  gms.  95%  alcohol  dissolve  0.00275  gm.  PbC4H4O4  at  18°,  and 
0.003  gm-  at  25°- 

Density  of  alcohol  used  =  0.8092. 

LEAD    SULPHATE    PbSO4. 

One  liter  of  water  dissolves  0.041  gm.  PbSO4,  by  conductivity 
method. 

(Kohlrausch;  Bottger.    Dibbits  —  Z.  anal.  Chem.  13,  1.39,  '74,  finds  0.038  gram  by  gravimetric  method.) 

SOLUBILITY  OF  LEAD  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF  STRONG 

ACIDS. 

(Schultz  —  Pogg.  Ann.  113,  137,  '61;  Rodwell  —  J.  Chem.  Soc.  15,  59,  '62.) 

In  Aq.  H2SO4.  In  Aq.  HC1.  In  Aq.  HNO3. 

(a).  (6).  (c).  (a).  (6).  (c).  (a).          (6).  (c). 

1.540     63.4    0.003  1.05     10.6     0.14  i. 08     i i. 6     0.33 

1-793  85.7  o-o11    I-o8  l6-3  °-35  J-12  J7-5  °-59 

1.841  97.0  0.039    i. ii  22. o  0.95  1.25  34-0  0.78 

1.14  27.5  2. ii  1.42  60.0  i.oi 

1.16  31.6  2.86 

(a)  Sp.  Gr.  of  Aq.  Acid,  (i)  Gms.  Acid  per  ioo  Gms.  Solution,   (c)  Gms.PbSO*  per  ioo  Gms.  Solvent. 


SOLUBILITY   OF   LEAD   SULPHATE   IN  AQUEOUS  SOLUTIONS  OF  AMMO- 
NIUM ACETATE  AND  OF  SODIUM  ACETATE. 

(Noyes  and  Whitcomb  —  J.  Am.  Chem.  Soc.  27,  756,  '05;  Dunnington  and  Long  —  Am.  Ch.  J.  22, 
217,  '99;  Dibbits  —  Z.  anal.  Chem.  13,  139,  '74.) 

In  Ammonium  Acetate.  In  Sodium  Acetate. 

At  25°  (N.  and  W.).  At  100°  (D.  and  L.).  (D.). 


1  
Millimols 

per  Liter. 

Grams  per  Liter.        G. 

NH4C2H302  G.PbSO4 

Gms.  per  ioo  Gms.  H2O. 

NH4C2H302.    PbS04.        NH^HsOa. 

PbSO,       ^solution. 

Solution. 

NaC2H3O2.    PbSO4. 

O-O 

0.134 

O-O 

O.O4I 

28 

7-12 

2.05 

0.054 

I03.S 

2.10 

7.98 

0.636 

32 

9.88 

8.2 

0.853 

207.1 

4-55 

I5-96 

1.38 

37 

10.58 

41.0 

II  .23 

4I4.I 

10.  IO 

31.92 

3-02 

45 

II  .IO 

LEAD    (Hypo)    SULPHATE         170 

SOLUBILITY  OF  MIXTURES  OF  LEAD  HYPOSULPHATE  AND  STRONTIUM 
HYPOSULPHATE  AT  25°. 

(Fock  — Z.  Kryst.  Min.  28.  389,  '97.) 


il.  per  cent  in  Solution. 

Grams  per  Liter. 

Sp.  Gr.  of 

Mol.  per  cent  in  Solid  Phase 

PbS^o           SrSaOa               PbS2Oe.          SrS2Oe- 

Solutions.           PbS^Oe 

SrS206 

-4H2O. 

.4H 

-4H20. 

.4H20. 

0-0 

IOO 

.0 

O 

.0 

145 

6 

I 

.1126 

0 

.0 

IOO.O 

1.05 

98 

•95 

2 

•97 

.2 

I 

.1184 

O 

•30 

99  7 

84 

.69 

40 

.82 

152 

•5 

I 

.1503 

3 

.87 

96.13 

46.80 

53 

.20 

149 

.2 

114 

•5 

I 

.2147 

9 

.84 

90.16 

62.30 

37 

.70 

256 

.1 

85 

.0 

I 

.2889 

19 

.26 

80.74 

75-75 

24 

•25 

3IO 

•3 

67 

.0 

I 

•3252 

23 

•73 

76.27 

78.09 

21 

.91 

373 

•7 

70 

.8 

I 

.3726 

32 

.24 

67.76 

88.29 

II 

•71 

509 

•5 

45 

.6 

I 

.4671 

49 

•97 

50.13 

IOO.O 

O 

.00 

374 

•3 

0 

.0 

I 

.6817 

0 

.00 

o.oo 

LEAD    TARTRATE    PbC4O6H4. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder  —  Bull.  soc.  chim.  [3]  33,  751,  '05;   Partheil  and  Hiibner  —  Archiv.  Pharm.  241, 

413,  '03-) 


to         Cms.  PbCiOeHi  Per  1  0  Cms.  PbC4O6H4  per  ±0        Gms.  PbC4O6H4  per 

100  cc.  Solution.  ioo  cc.  Solution.  100  cc.  Solution. 

l8       O-OIO   (P.  andH.)  50       O-OO225         70       0.0032 

25  0.0108  "  55  0.00295  75  0.0033 
35  0.00105  60  0.00305  80  0.0038 
40  0.0015  65  0.00315  85  0-0054 

NOTE.  —  The  positions  of  the  decimal  points  here  shown  are  just 
as  given  in  the  original  communications. 

100  gms.  alcohol  of  0.8092  Sp.  Gr.  (about  95%)  dissolve  0.0028  gm. 
PbC4O6H4at  1  8°,  and  0.003  1  5  gm-  at  25°-  (P.  and  H.) 

LEVULOSE    C6H12O6. 

100  gms.  saturated  solution  in  pyridine  contain  18.49  gms-  C6H12Oa 

at  26°,  Sp.  Gr.    1.0521.  (Holty  —  J.  Physic.  Chem.  g,  764,  '05.) 

LIGROIN. 

ioo  cc.  H2O  dissolve  0.341  cc.  ligroin  at  22°  Vol.  of  solution  =  100.34, 
Sp.  Gr.  0.9969. 

ioo  cc.  ligroin  dissolve  0.335  cc.  H2O  at  22°  Vol.  of  solution  =  100:60, 

Sp.  Gr.  0.6640.  (Herz—  Ber.3i,  2671,  '98.) 

LITHIUM    BENZOATE    C6H5COOLi. 

ioo  gms.  H2O  dissolve  33.3  gms.  at  25°,  and  40.0  gms.  at  b.  pt. 
ioo  gms.  alcohol  dissolve  7.7  gms.  at  25°,  and  10.0  gms.  at  b.  pt. 

(U.  S.  P.) 

LITHIUM    BORATE    Li2OB2O3. 

SOLUBILITY  IN  WATER. 

t°  o         10        20        30        40        45 

Gms.  Li2OB2O3  per  ioo  Gms.  H2O     0.7       1.4      2.6      4.9     11.12  20 

(Le  Chatelier  —  Compt.  rend.  124,  1094,  *97-) 


iyi  LITHIUM    BROMATE 

LITHIUM    BROMATE    LiBrO3. 

100  gms.  H2O  dissolve  153.7  gms.  LiBrO3  at  18°,  or  100  gms.  saturated 
solution  contain  60.4  gms.  Sp.  Gr.  of  sol.  =  1.833. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 

LITHIUM    BROMIDE    LiBr. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg.  Ann.  104,  133,  '58.) 
0       Gms.  LiBr  per  100  Gms.  Gms.  LiBr  per  100  Gms. 

Water.        Solution.  Water.         Solution. 

O  143  58.8  40  202  66.9 

10         161         61.7  50        214        68.2 

2O     177     63.9  60     224     69.1 

25      184     64.8  80     245     71.0 

30         190         65.5  ioo         266         72.7 

ioo  gms.  saturated  solution  in  glycol,  C2H4(OH)2.H2O,  contain  37.5 

gms.  LiBr  at  14.7°.  (de  Coninck  —  Chem.  Centr.  76,  II,  883,  '05.) 

LITHIUM    CARBONATE    Li2CO3. 

SOLUBILITY  IN  WATER. 

(Bevade  —  J.  russ.  phys.  chem.  Ges.  16,  591,  84;  Bull.  soc.  chim.  [2]  43,  123,  '85;  Fliickiger  —  Arch. 
Pharm.[3]25,  542,  '87;  Draper  —  Chem.  News,  55,  169,  '87.) 

An  average  curve  was  constructed  from  the  available  results  and 
the  following  table  read  from  it. 

Gms.  Li2CO3  per  ioo  Gms.  0        Gms.Li2CO3  per  looGms. 

Water.          Solution.  Water.          Solution. 

o  .54         1.52  40         1.17         1.16 

10  .43         1.41  50         i.  08         1.07 

20  .33  1.31  60  I.  01  I.  00 

25  .29  1.28  80  0.85  0.84 

30  .25         1.24  ioo        0.72         0.71 

Density  of  saturated  solution  at  o°  =  1.017;  at  15°  =  1.014. 

SOLUBILITY  OF  LITHIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OP 
ALKALI  SALTS  AT  25°. 

(Geffcken  —  Z.  anorg.  Chem.  43,  197,  '05.) 

The  original  results  were  calculated  to  gram  quantities  and  plotted 
on  cross-section  paper.  The  figures  in  the  following  table  were  read 
from  the  curves. 

Gms.  Salt  Grams  Li2CO3  per  Liter  in  Aqueous  Solutions  of: 


per  Liter. 

KC 

KNOg. 

KC1. 

NaCl. 

K2S04. 

Na2S04. 

NH4C1. 

(NH4)2S04. 

O 

12 

•63 

12.63 

12  .63 

12 

.63 

12  .63 

12 

.63 

12.63 

12.63 

10 

12 

•95 

I  3  •  O'N 

13  .IO 

13 

•4 

13-9 

14 

•  o 

16.0 

20-7 

2O 

I3 

.10 

13-3 

13-5 

*3 

•9 

14.7 

15 

•  o 

19.2 

25.0 

30 

13 

•25 

13-6 

I3.8 

14 

•3 

IS-4 

16 

.0 

21.5 

28.2 

40 

13 

.40 

I3.8 

14.0 

14 

.6 

16.0 

16 

.6 

23-3 

30.8 

60 

I3.8 

14-2 

14 

•5 

16.9 

i? 

.8 

.  26.0 

35-2 

80 

. 

13-6 

14.0 

14 

•4 

17.7 

18 

.6 

27.6 

38-5 

IOO 

. 

J3-5 

J3-9 

14 

.  2 

18.2 

19 

4 

28.4 

41.0 

120 

. 

13-3 

13-7 

14 

•  O 

19 

9 

28.7 

42.6 

140 

. 

13.0 

13-3 

. 

20 

4 

28.8 

43-5 

170 

. 

12.6 

28.9 

2OO 

12  .2 

20  .0 

ioo  gms.  aq.  alcohol  of  0.941  Sp.  Gr.  dissolve  0.056  gm.  Li2CO3  at 


LITHIUM    (Bi)    CARBONATE       172 
LITHIUM    (Bi)    CARBONATE    LiHCO3. 

100  grams  H2O  dissolve  5.501  grams  LiHCO3  at  13°. 

(Bevade  —  Ber.  17,  R  406,  '84.) 

LITHIUM    CHLORATE    LiClO3. 

100  grams  H2O  dissolve  213.5  grams  LiClO3  at  18°,  or  100  grams  sat. 
solution  contain  75.8  grams.     Sp.  Gr.  of  sol.  =  1.815. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 

LITHIUM    CHLORAURATE    LiAuCl4. 

SOLUBILITY  IN  WATER. 

(Rosenbladt  —  Ber.  19,  2538,  '86.) 


A  o        Gms.  LiAuCU  per           +  0        Gms.  LiAuCU  per 
TOO  Gms.  Solution.                      100  Gms.  Solution 

I  o   Gms.  LiAuCU  per 
100  Gms.  Solution. 

10 

53-i 

40 

67-3 

60 

76.4 

20 

57-7 

50 

72.0 

70 

81.0 

30 

62  .5 

80 

85.7 

LITHIUM    CHLORIDE    LiCl. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Gerlach  —  Z.  anal.  Chem.  8,  281,  '69.) 

Gms.  LiCl  per  100  Gms.  ^  Gms.  LiCl  yr  100  Gms. 

Water.  Solution."  Water.  Solution. 

o  67  40.1  40  90.5  47.5 

10  72  41.9  50  97.0  49.2 

20  78.5  44 -o  60  103.0  5z-9 

25  81.5  49.9  80  115.0  53.5 

30  84.5  45.8  100  127.5  56-° 

Density  of  saturated  solution  at  o°,  1.255;  at  I5°»  I-275- 

SOLUBILITY  OF  LITHIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF  HYDRO- 
CHLORIC ACID  AT  o°. 

(Engel  —  Ann.  chim.  phys.  [6]  13,  385,  '88.) 


Milligram  Mols.  per 
10  cc.  Solution. 

Gms.  per  10  cc. 
Solution. 

Sp.  Gr.  of 

LiCl. 

HCl. 

LiCl. 

HCl.' 

Solutions. 

1  2O 

o.o 

5I.O 

0-0 

1-255 

97-5 

22  .5 

41.4 

8.2 

1.243 

67.0 

66.0 

28.5 

24.1 

1.249 

58.0 

81.0 

24.6 

29-5 

I  .251 

SOLUBILITY  OF  LITHIUM  CHLORIDE  IN  SEVERAL  SOLVENTS. 

(von  Laszczynski  —  Ber.  27,  2285,  '94;  de  Coninck  —  Chem.  Centrh.  76,  II,  883,  '05.) 


Gms.  LiCl 
t  °.    per  100  Gms. 
(CH3)2CO. 

o        4.60 

12  4.41 

2$  4-II 


etoi 

L.) 

ne. 

In  Pyridine. 

(von  L.) 

In  Glycol. 

(de  C.) 

Gms.  LiCl 

Gms.  LiCl 

Gms.  LiCl 

t  °. 

per  100  Gms. 

t  °.        per  100  Gms. 

t°.     per  100  Gms. 

(CH3)2CO. 

C6H6N. 

Sat.  Sol. 

46 

3.76 

15°              7-78 

15°      ii.  o 

53 

3-12 

100         14.26 

58 

2.14 

173 
LITHIUM    CHROMATE    Li2CrO4.2H2O. 


LITHIUM    CHROMATE 


LITHIUM    BICHROMATE    Li2Cr2O7.2H2O. 

SOLUBILITY  IN  WATER  AT  30°. 

(Schreinemaker  —  Z.  physik.  Chem.  55,  79,  '06;  at  1 8°,  Mylius  and  Funk  —  Ber.  30,  1718, '97.) 

Composition  in  Weight  per  cent: 

Solid 
Phase. 

LiOH.H2O 


LiOH.H20  +  Li2Cr04.2H2O 


Of  Solution. 

Of  Residue. 

%Cr03. 

%Li20. 

%Cr03. 

%Li20. 

o.o 

7.09 

6.986 

7-744 

4.322 

18.538 

16.564 

8.888 

10-089 

I9-556 

25.811 

10.611 

15-479 

21  .106 

33-6l8 

12.886 

24-365 

19.398 

37-4H 

14.306 

44-555 

17.411 

37-588 

14.381 

36-331 

18.552 

37-495 

13-3" 

5i-o75 

16.384 

40  .  280 

10.858 

43.404 

i  i  .  809 

53-793 

14.070 

45  -13° 

9-5*5 

56.085 

10.190 

47-945 

7-951 

58.029 

9.238 

57-Q31 

6.432 

65.560 

8-733 

67.731 

5-7I3 

71.687 

8-5I3 

67.814 

5-689 

80.452 

3.780 

65  .  200 

4.661 

.  .  . 

63-257 

2.141 

85.914 

0.758 

62.28 

Li2CrO4.2H2O 


Li2Cr2O4.2 


Li2Cr207.2H2O 


Li2Cr207.2H20  +  Cr03 


Cr03 


A  saturated  aqueous  solution  contains : 

49.985  per  cent   Li2CrO4,  or  100  grams  H2O   dissolve   99.94  grams 
Li2CrO4  at  30°  (S.). 

56.6   per  cent   Li2Cr2O7,  or    100   grams  H2O   dissolve   130.4   grams 
Li2Cr2O7  at  30°  (S.). 

52.6    per  cent    Li2CrO4,   or    100   grams  H2O  dissolve   110.9 
LiCrO4at  18°  (M.  and  F.). 

Sp.  Gr.  of  sat.  solution  at  18°  =  1.5 74. 


LITHIUM    CITRATE    C3H4(OH)(COOLi)3. 

100  gms.  H2O  dissolve  50  gms.  citrate  at  25°,  and  66.6  gms.at  b.  pt. 
100  gms.  alcohol  of  0.941  Sp.  Gr.  dissolve  4  gms.  citrate  at  15.5°. 

(U.  S.  P.) 


LITHIUM    FLUORIDE    LiF. 

100  grams  H2O  dissolve  0.27  gram  LiF  at  18°.     Sp.  Gr.  of  sol.  «» 
1.003. 

(Mylius  and  Funk.) 


LITHIUM  FORMATE 


174 


LITHIUM    FORMATE    HCOOLi. 


SOLUBILITY  IN  WATER. 

(Groschuff  —  Ber.  36,  179,  '03.) 


Gms. 

Mols. 

Gms. 

Mols. 

HCOOLi 

HCOOLi 

Solid 

HCOOLi 

HCOOLi 

Solid 

per  ioo 

per  ioo 

Phase. 

t  °. 

per  ioo 

per  ioo 

Phase. 

Gms. 

Mols. 

Gms. 

Mols. 

Solution. 

H20. 

H20. 

H20. 

21  .14 

9.28 

HCOOLi  .H20 

91 

54.16 

40.90 

HCOOLi  .H20 

24.42 

II.  l8 

" 

98 

57-05 

45-99 

HCOOLi 

27.85 

13-36 

" 

104 

57  -°4 

47.11 

" 

35  -60 

19.14 

11 

120 

59-63 

51  .13 

" 

44.91 

28.22 

" 

—  20 
O 

18 

49-5 
74 

Sp.  Gr.  sat.  sol.  at  18°  =  1.142. 


SOLUBILITY  OF  NEUTRAL  LITHIUM  FORMATE  IN  ANHYDROUS 
FORMIC  ACID. 


Gms.  per  100  Gms.  Solution. 


Mols.  per  TOO  Mols.  H2O. 


V        . 

HCOOLi. 

HCOOH. 

HCOOLi. 

HCOOH. 

O 

25-4 

47-02 

II.So 

39-27 

18 

25-9 

46.92 

12.  1  1 

39-11 

39 

26.4 

46.92 

12  .42 

39  -13 

60 

26.9 

46.94 

12-74 

39-13 

79 

27.8 

47-02 

I3-36 

39.26 

HCOOLi 


LITHIUM    HYDROXIDE    LiOH. 

SOLUBILITY  IN  WATER. 

(Dittmar  —  J.  Soc.  Ch.  Ind.  7,  730,  '88;  Pickering  — J.  Chem.  Soc.  63,  909,  '93.) 


Gms.  per 

ioo  Gms. 

Gms.  LiOH 

Gms.  per  ioo  Gms. 

Gms.  LiOH. 

t° 

Solution. 

per  ioo  Gms. 

t°.                      Solution. 

per  ioo  Gms 

Li20. 

LiOH. 

H2O. 

Li2O. 

LiOH. 

H20. 

O 

6.67 

10.64 

12-7 

40 

7.29 

11.68 

I3.0 

IO 

6.74 

I0.8o 

12-7 

50 

7-56 

12.12 

20 

6.86 

10-99 

12.8 

60 

7.96 

12.76 

13  :1 

25 

6-95 

II  .14 

12-9 

80 

8.87 

14.21 

15-3 

30     7-05 


11.27 


12.9 


IOO       10. O2 


16.05      17-5 


LITHIUM    IODATE    Li(IO3). 

ioo  grams  H2O  dissolve  80.3  grams  LiIO3  at  18°,  or  ioo  grams  solu- 
tion contain  44.6  grams.     Sp.  Gr.  of  sol.  =  1.568. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 


Water. 

Solution. 

\>       * 

Water. 

Solution. 

151 

60.2 

40 

179 

64.2 

J57 

61.1 

50 

I87 

65-2 

62  .2 

60 

202 

66.9 

167 

62.6 

70 

230 

69.7 

171 

63.I 

75 

263 

72-5 

175  LITHIUM   IODIDE 

LITHIUM    IODIDE    Lil. 

SOLUBILITY  IN  WATER. 

(Kremefs  —  Pogg.  Ann.  104,  133,  '58;  in,  60,  '60.) 
0  Gms.  Lil  per  ioo  Gms.  ^  0  Grams  Lil  per  ioo  Gms. 

O 
10 
2O 

25 

30 

ioo  grams  sat.  solution   in   Glycol    (C2H4(OH)2.H2O)    contain    28.0 

grams  Lil  at  15.3°.  (de  Coninck  —  Chem.  Centrb.  76,  II,  883,  '05.) 

ioo  cc.  saturated  solution  in  Furfurol  (C4H3O.COH)  contain  45.86 
gms.  Lil  at  25°. 

ioo  cc.  saturated  solution  in  Nitro  Methane  (CH3NO2)  contain 
1.219  gms-  Lil  at  o°,  and  2.519  gms.  at  25°. 

(Walden  — Z.  physik.  Ch.  55,  713,  718,  '06.) 

LITHIUM    NITRATE    LiNO3. 

SOLUBILITY  IN  WATER. 

(Donnan  and  Burt  —  J.  Chem.  Soc.  83,  335,  '03.) 

to        Gms.LiNOaper  Solid  to        Gms.  LiNO3  per  Solid 

ioo  Gms.  Solution.         Phase.  ioo  Gms.  Solution.          Phase. 

O.I  34-8  LiN03.3H2O  29.87  56.42          LiN03.3H20 

10-5  37.9  "  29.86  56.68 

12. I  38.2  "  29.64  57-48 

13-75        39-3  "  29.55        58-03 

19.05  40.4  43-6  60.8  LiN03.*H2O 

21- 1  42-9  "  5°-5  61.3 

27-55        47-3               "                 55-o  63.0 

29-47        53-67             "                 6o-°  63-6 

29-78        55-09             "                 64-2  64.9 

70.9  66.1 

Cryohydrate  point  of  the  trihydrate,  17.8°.  Transition  points,  29.6° 
and  61.1°. 

LITHIUM    OXALATE    Li2C2O4. 

SOLUBILITY  OF  MIXTURES  OF  LITHIUM  OXALATE  AND  OXALIC 
ACID   IN  WATER  AT  25°. 

(Foote  and  Andrew  —  Am.  Ch.  J.  34,  153,  '05.) 

Mixtures  of  the  two  substances  were  dissolved  in  water,  and  the 
solutions  cooled  in  a  thermostadt  to  25°. 

Gms.  per  ioo  Gms.  Solution.       Mols.  per  ioo  Mols.  H2O.  Soli(j 

H2C204.        Li2C204.  H2C204.        Li2C204.'  Phase. 

10 . 20  ...  2  . 274  H2C204.2H2O 

10 .66       2 .06  s 

2.457  0.622  H2C204.H20  and  HLiC2O4.H2O 

8.08         3-18  1.823  0.633)  Double  Salt 

2.60         5.03  0.563  0.962J  H=3f24H42?204  and  44-7  Li2C20, 

2    12         I 'III  0.469  1-273  HLiC204.H20  and  U2C204 

5.87  ...  I.90I  Li2C204 


LITHIUM    PHOSPHATE  176 

LITHIUM    PHOSPHATE    Li3PO4. 

100  grams  H2O  dissolve  0.04  gram  L13PO4.  (Mayer  —  Liebig's  Ann. 98, 193, '56.) 

LITHIUM    (Hypo)    PHOSPHATE    Li4P2O6.7H2O. 

100  grams  H2O  dissolve  0.83  gram  hypophosphate  at  ord.  temp. 

(Rammelsberg  —  J.  pr.  Ch.  [2]  45,  153,  '92.) 

LITHIUM    PERMANGANATE    LiMnO4.3H2O. 

100  grams  water  dissolve  71.4  grams  permanganate  at  16°. 

(Ashoff.) 

LITHIUM    SALTS    of  Fatty  Acids. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL  OF  0.797  SP.  GR.  AT  18° 

AND    AT    25°. 
(Partheil  and  Ferie  —  Archiv.  Pharm.  241,  554,  '03.) 

Grams  Salt  per  100  cc.  Sat.  Solution  in: 


Salt. 

Stearate 
Palmitate 
Myristate 
Laurinate 
Oleate 

Formula. 

C17H35COOLi 
C15H31COOLi 
C13H27COOLi 
CnH23COOLi 

C^HggCOOLi 

Water  at 

Alcohol  at 

0 
0 
0 
0 
0 

18°. 
•  OIO 
.Oil 

.0232 

.158 

.0674 

o 

0 
0 

o 
o 

25°. 
•  Oil 

.018 
.0234 
.1726 
.1320 

'  18°. 
O.O4I 
0.0796 
0.184 
0.418 
0.9084 

0 
O 
O 
0 

I 

25°. 

•0532 
.0956 
.2IOO 
.4424 
•  OIO 

LITHIUM    SULPHATE    Li2SO4. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  Kremers  —  Pogg.  Ann.  95,  468,  '55;  Etard  —  Ann.  chim.  phys.  [7]  2,  547,  '94.) 


j.o            Gms.  Li2SO4  per 
100  Gms.  Solution 

j.o          Gms.  Li2SO4  per 
100  Gms.  Solution 

4.0          Gms.  Li2SO4  per 
.                           100  Gms.  Solution. 

—  20 

18.4 

20 

25-5 

50 

24-5 

—  10 

24.2 

25 

25-3 

60 

24.2 

O 

26.1 

30 

25-1 

80 

23-5 

10 

25-9 

40 

24.7 

100 

23.0 

NOTE.  —  For  equilibrium  between  lithium  sulphate  ammonia  and 
water,  see  Schreinemaker  and  Cochert  —  Chem.  Weekblad.  2,  771;  3, 
157,  '06. 

EQUILIBRIUM  BETWEEN  LITHIUM  SULPHATE,  ALUMINUM  SULPHATE, 
AND  WATER  AT  30°. 

(Schreinemaker  and  De  Waal  —  Chem.  Weekblad.  3,  539,  '06.) 
Composition  in  Weight  per  cent: 


Of  Solution. 

Of 

Residue. 

Solid 
Phase. 

%  Li2SO4.            % 

A12(S04)3. 

%  Li2SO4 

,        %  A12(S04)3. 

25.1 

O 

Li2SO4.H2O 

21-93 

5-34 

" 

16.10 

14.89 

63.70 

4-O2 

« 

13-63 

20.76 

14.72 

3I-I7 

(  Li2S04.H20  + 
1      Al2(SO4)3.i8H2O 

13.24 

21.71 

61  .24 

7-22 

Li2S04.4H2O 

ii  .73 

22  .08 

6.92 

33-54 

Al2(SO4)3.i8H2O 

6-75 

24-34 

3-77 

37.06 

M 

3-44 

26.12 

«« 

o.o 

28.0 

.  .  . 

1. 

NOTE.  —  For  solubility  of  lithium  sulphate  in  mixtures  of  alcohol 
and  water  at  30°,  see  Schreinemaker  and  Van  Dorp,  Jr.  —  Chem.  Week- 
blad. 3,  557,  '06. 


177  MAGNESIUM    BROMATE 

MAGNESIUM    BROMATE    Mg(BrO3)2.6H2O. 

100  cc.  sat.  solution  contain  42  grams  Mg(BrO3)2,  or  0.15  grammols. 
at  1 8°. 

(Kohlrausch  — Sitzb.  K.  Akad.  Wiss.  (Berlin),  i,  90,  '07.) 

MAGNESIUM    BROMIDE    MgBr2.6H2O. 

SOLUBILITY  IN  WATER. 

(Menschutkin  —  Chem.  Centrb.  77,  I,  646,  '06;  at  18°,  Mylius  and  Fu.ik —  Ber.  30,  1718,  '97.) 

0        Grams  MgBij  per  100  Gms.  0      Grams  MgBr2per  100  Grams. 

Solution.  Water.  Solution.         Water. 

—  io  47.2  89.4  40  50.4  101.6 

o  47-9  91 -9  50  51-0  104.1 

io  48.6  94.5  60  51.8  107.5 

18  49-0  96.1  80  53-2  JI3-7 

18  50.8  103 .4  (M.  and  F.)     100  54-6  120.2 

20  49.1  96.5  120  56.0  127.5 

25  49.4  97.6  140  58.0  138.1 

30  49-8  99-2  160  62.0  163.1 

Density  of  saturated  solution  at  18°  =  1.655  (M.  and  F.) 
Etard  —  Ann.   chim.   phys.    [7]   2,  541,  '94,  gives  solubility  results 
which  are  evidently  too  high. 

SOLUBILITY  OF  MAGNESIUM  BROMIDE  ALCOHOL  COMPOUNDS  IN  THE 
CORRESPONDING  ALCOHOLS. 

(Menschutkin  —  Chem.  Centrb.  77,  I,  334,  647,  '06.) 

In  the  Corresponding  Alcohols. 

Results  Expressed  in  Mols.  per  cent. 


t<>. 

MgBr2.6CH3OH 
in  CH3OH. 

MgBr2.6C2H5OH 
in  C2H6OH. 

0 

6.0 

2.O 

20 

6.4 

4-6 

40 

6.9 

8.4 

50 

7.2 

IO-9 

60 

7-5 

I4-I 

80 

8.25 

22.1 

100 

9.6 

38.6 

150 

16.7 

100.0  (108. 

5°) 

i  go 

IOO.O 

Determinations  are  also  given  for  the  solubility  of  MgBr2.6C3H7OH 
in  C3H7OH,  of  MgBr2.6(CH3)2C2H3OH  in  (CH3)2C2H3.OH,  and  of  MgBr2. 
6(CH3)2C2H3OH  in  (CH3)2C2H3OH,  also  of  MgBr2.4(CH3)2.CHOH  in 
iso  propyl  alcohol  and  in  tri  methyl  carbinol. 

For  the  solubility  magnesium  bromide  mono  etherate  (MgBr2. 
(C2H6)2O)  in  ethyl  ether,  see  Menschutkin  —  Chem.  Centrb.  77, 1,  1868, 
'06;  also  Z.  anorg.  Ch.  49,  208,  '06.  For  magnesium  bromide  di 
etherate  (MgBr2.2C4H10O)  in  ethyl  ether,  see  Menschutkin  —  Z.  anorg. 
Ch.  49,  35,  '06.  For  magnesium  bromide  hexa  formic  acid  and  mag- 
nesium bromide  hexa  acetic  acid  compounds  in  anhydrous  solutions  of 
the  corresponding  acids,  see  Iswietja  d.  Petersburger,  Polytechn.  Inst. 
6,  293,  '06;  Chem.  Centrb.  77,  II,  1482,  '06. 


MAGNESIUM    CARBONATE       178 
MAGNESIUM    CARBONATE    MgCO3. 

SOLUBILITY  IN  WATER  IN  PRESENCE  OF  CARBON   DIOXIDE   AT   15* 

(Tread well  and  Reuter  —  Z.  anorg.  Ch.  17,  200,  '98.) 


cc  CO2  t>er  TOO  cc- 
Gas  Phase  (at  o° 

Partial 
Pressure  of  COs 

Grams  per 

ioo  cc.  Solution. 

and  760  mm.)- 

in  mm.  Hg. 

Free  CO2. 

MgCO3. 

Mg(HC03)2. 

Total  Mg. 

18.86 

143-3 

O.II90 

.  .  . 

I  .2IO5 

0.2016 

5-47 

41  .6 

0.0866 

I  .2IO5 

0.2016 

4-47 

33-8 

0.0035 

I.2I05 

0.2016 

i-54 

11.7 

0.0773 

I  .0766 

0.2016 

J-35 

10.3 

0.0765 

0.7629 

0.1492 

1.07 

8.2 

0.0807 

0-5952 

0.1224 

0.62 

4-7 

O.O7OI 

0.3663 

0.0865 

0.60 

4.6 

0.0758 

0.3417 

0.0788 

o-33 

2-5 

0.0748 

0.2632 

0.0655 

0.21 

1.6 

0.0771 

O.2229 

0.0594 

O.I4 

i  .1 

O.O7IO 

0.2169 

0.0566 

O.O3 

o-3 

O.O7II 

0-2036 

0-0545 

0.0685 

0.2033 

0-0536 

O.O7O2 

0.1960 

0.0529 

0.0625 

0.2036 

0.0520 

0.0616 

0.1954 

0.0511 

0.0641 

0.1954 

0.0518 

Therefore  at  o  partial  pressure  of  CO2  and  at  1 5°  and  mean  barometric 
pressure,  one  liter  of  saturated  aqueous  solution  contains  0.641  gram 
of  MgCO3  plus  1.954  grams  Mg(HCO3)2. 


SOLUBILITY  OF  MAGNESIUM  CARBONATE  IN  WATER  CHARGED  WITH  CAR- 
BON DIOXIDE  AT  PRESSURES  GREATER  THAN  ONE  ATMOSPHERE. 

(Engel  and  Ville  —  Compt.  rend.  93,  340.  '81;  Engel  — Ann.  chim.  phys.  [6]  13,  349,  '88.) 


Pressure  of 
CC>2  in 

G.  MsCOa^ 

per  Liter. 

Pressure  of 

f~*O      in 

G.  MRCO3*  per  Liter. 

Atmospheres. 

At 

12°. 

At  19°. 

LxV_/2  1" 

Atmospheres  0 

At    12°. 

At  19°. 

0-5 

20. 

5 

4 

.0 

42.8 

I  .0 

26. 

5 

25 

.8 

4 

•7 

43-5 

2-0 

34- 

2 

33 

.1(2, 

i  At.) 

6 

.0 

5O.6 

48-5 

(6.2 

At.) 

3-o 

39- 

O 

37 

•2(3 

.2  At.) 

9 

.0 

56.6 

SOLUBILITY  IN  WATER  SATURATED  WITH  CO2  AT  ONE  ATMOSPHERE. 

(Engel.) 

to          Cms.  MgCO3*  f0         Gms.MgCOa*  ..<,  Cms.  MgCO3* 

per  Liter.  per  Liter.  per  Liter. 

5     36       30     21  60     ii 

10     31       40     17  80      5 

20     26  ioo      o 

*  Dissolved  as  Mg(HCO3)2. 


179       MAGNESIUM    CARBONATE 

SOLUBILITY  OP  MAGNESIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OP 
SODIUM  CARBONATE  AT  25°.  The  solutions  being  in  equilibrium 
with  an  atmosphere  free  from  CO2. 

(Cameron  and  Seidell  —  J.  Physic.  Ch.  7,  588,  '03.) 

Wt.  of  i  Liter  Grams  per  Liter.  Reacting  Weights  per  Liter. 

of  Solution.  Na2C03.  MgCO3.  Na2CO3.  MgCO3'. 

996.8       o.oo     0.223     o.ooo     0.00266 


1019.9 

23.12 

0.288 

O-22O 

0.00344 

1047.7 

50-75 

0.510 

0.482 

O.O062O 

1082.5 

86.42 

0.879 

O.82O 

O.OI027 

1118.9 

127.3 

i  -3*4 

I  .209 

O.OI57O 

1147.7 

160.8 

1.636 

I  .526 

0.01955 

1166.1 

181.9 

1.972 

1.727 

0.02357 

1189.4     213.2      2.317     2.024     0.02770 


SOLUBILITY  OF  MAGNESIUM  Bi  CARBONATE  AND  OF  MAGNESIUM  CAR- 
BONATE IN  AQUEOUS  SOLUTIONS  OF  SODIUM  CHLORIDE  AT  23°.  The 
solutions  being  in  equilibrium  with  an  atmosphere  of  CO2  in  the 
one  case,  and  in  equilibrium  with  air  free  from  CO2  in  the  other. 

(C.  and  S.) 
In  Presence  of  CO2  as  Gas  Phase. 


Gms.  NaCl 
per  Liter. 

Gms,  Mg(HC03)2 
per  Liter. 

Wt.  of  i 
Liter. 

Gms.  NaCl 
per  Liter. 

Gms.  MgCO3 
per  Liter. 

7-0 

30.64 

996.9 

0.0 

0.176 

56.5 

30.18 

IOI6.8 

28.0 

0.418 

119.7 

27.88 

IO4I  .1 

59-5 

0.527 

163.9 

24.96 

1070.5 

106.3 

0.585 

224.8 

20.78 

1094-5 

147-4 

0-544 

306.6 

10-75 

1142.5 

23I.I 

0.460 

II7O.I 

272.9 

o-393 

II99-3 

331-4 

0.293 

SOLUBILITY  OF  MAGNESIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  SULPHATE  AT  24°  AND  AT  35.5°.  The  solutions  being  in 
equilibrium  with  an  atmosphere  free  from  CO2. 

(Cameron  and  Seidell.) 

Results  at  24°.  Results  at  35.5.° 


Wt.  of 

Gms.  Na2SO4 

Gms.  MgCO3 

Wt.  of 

Gms.  Na2SO< 

Gms.  MgCO3 

i  Liter. 

per  Liter. 

per  Liter. 

i  Liter. 

per  Liter. 

per  Liter. 

997-5 

o.oo 

0.216 

995  -1 

0-32 

O.I3I 

IO2I  .2 

25.12 

0.586 

1032.9 

41.84 

o-577 

1047.6 

54  76 

0.828 

1067.2 

81.84 

0.753 

1080.9 

95.68 

I  .020 

1094.8 

116.56 

0.904 

1133  .8 

160.8 

1.230 

1120.4 

148.56 

0.962 

"57-3 

191.9 

1.280 

1151  .7 

186.7 

1.047 

1206.0 

254.6 

I-338 

1179.8 

224.0 

i.  088 

1242.0 

305-1 

I.388 

1236-5 

299.2 

1.130 

MAGNESIUM    CHLORATE 


1 80 


MAGNESIUM    CHLORATE    Mg(ClO3)5 


i8 

0 

18 
29 

35 

Gms. 
Mg(C103)2 
per  100  Gms, 
Solution. 

51.64 
53-27 

60.23 

Mols. 
Mg(C103)2 
,    per  100 
Mols.  H2O. 

IO.O5 
10-73 
12.22 
14.25 
16.48 

SOLUBILITY 

(Meusser  —  Ber. 

Solid 
Phase. 

Mg(C103)2.6H20 
ii 

IN 
35. 

t 

42 
65 

39 
61 
68 
93 

WATER. 
1416,  '02  .) 

Gms. 
o       Mg(C103)2 
°    per  loo  Gms. 
Solution. 

63.82 
•5      69.12 

•5     65.37 

•  O      69  .  46 
70.69 
(73-71) 

Mols. 
Mg(C103)2 
per  100 
Mols.H2O. 

16.16 

20.08 
17.76 
21.40 

22  .69 
(26.38) 

Solid. 
Phase. 

Mg(C103)2.4H20 
Mg(C103)a.2H20 

Sp.  Gr.  of  saturated  sol.  at  +  18°  =  1.564. 


MAGNESIUM    CHLORIDE    MgCl2. 

SOLUBILITY  IN  WATER. 

(van 't  Hoff  and  Meyerhoffer  —  Z.  physik.  Chem.  27,   75,   '98;  Engel;  Lowenherz.    Results  quoted 
from  Landolt  and  Bornstein —  Tabellen,  sd,  ed.  p.  549,  '06.) 


to  Gms.MgCl? 

per  TOO  Gms 

Solid 

40       Gms.  MgC^perioo 

Gms'  Solid 

Solution. 

Water. 

Phase. 

Solution 

.    Water. 

Phase. 

IO 

ii 

.1 

12 

•5 

Ice 

0 

34 

•5 

52 

.8 

MgCl2.6H2O 

20 

16 

.0 

19.0 

10 

34 

•9 

53 

•5 

" 

30 

19 

•4 

24.O 

2O 

35 

•3 

54 

•5 

33-6 

20 

.6 

26 

.0 

Ice  +  MgCl2.i2H2O 

22 

35 

.6 

55 

.2 

" 

12 

26 

•7 

36 

•5 

MgCl2.i2H2O 

25 

36 

.2 

56 

•7 

41 

16.4 

3° 

.6 

44 

.O4f.pt. 

40 

36 

•5 

57 

•5 

" 

16.8 
17.4 
19=4 
9.6 
3-4 

31 
32 
33 
33 
34 

.6 
-3 
•3 
•9 
•4 

46 
47 
49 
51 

S2 

2 

6 
9 
3 

3       j 

MgCl2.i2H2O  + 
MgCl2.8H2O  a 
MgCl2.i2H20  + 
MgCl2.8H20/3 
MgCl2.i2H20  + 
MgCl2.6H2O 
MgCl2.8H20  ft 
+  MgCl2.6H20 
MgClo.8H2O  a  + 
MgCl2.6H20      about 

60 
80 
100 
Il6.7 

152.6 
181.5 

37 
39 
42 

46 
49 

55 

•9 

.8 

.2 
.2 
.1 

.8 

61 

66 
73 
85 
96 
126 

.0 
.0 
.0 

•5 
•4 

.0 

(  MgCl2.6H20  -f 
1      MgCl2.4H2G 
MgCl2.4H20 
{  MgCl2.4H20  + 
\      MgCl2.2H20 

186 

56 

.1 

128 

.0 

MgCl2.2H20 

SOLUBILITY   OF   MAGNESIUM   CHLORIDE   IN   AQUEOUS   SOLUTIONS 
HYDROCHLORIC  ACID  AT  o°. 

(Engel — Compt.  rend.  104,  433,  '87.) 


gram  Mols.  p^r  10  cc.  Solution,     gp.  Gr.  of 

Grams  per  Liter  of  Solution. 

HC1. 

iMgC!2.              bolutions. 

HC1. 

MgCla. 

O-O 

99-55          1-362 

o.o 

474.2 

4-095 

95-5 

•354 

14-93 

454-8 

9-5 

90.0 

•344 

34-63 

428.6 

17.0 

82.5 

.300 

61.97 

393-o 

20.5 

79.0 

•297 

74-74 

376.2 

28.5 

71.0 

.281 

103.9 

338.3 

42.0 

60.125 

J53-i 

286.4 

58.75 

46.25 

214.2 

220.3 

76.0 

32.0 

277.1 

152.0 

sat.  HC1  (Ditte) 

6-S 

181          MAGNESIUM    CHLORIDE 

SOLUBILITY    OF    MIXTURES    OF   MAGNESIUM   CHLORIDE    AND    OTHER 
SALTS  IN  WATER  AT  25°. 

(LSwenherz —  Z.  physik.  Chem.  13,  479,  '94.) 

Mixture,  Gram  Mols.  per  1000  Mols.  H2O.      Gms.  per  Liter  of  Solution. 

MgCl2.6H2O  +  MgSO4.6H2O  104  MgCl2  + 14  MgSO4     25.0  C1  +  4.4  SO4 

MgCl2.7H20  +  MgS04.6H20  73  +15  19.5   "+5.3     " 

MgCl2.6H2O  +  MgCl2.KC1.6H2O     106  Cl+i  K2+  105  Mg     26.9  C1+ 0.3  K+ 45.7  SO4 

Results   for   the    remaining   possible    combinations   of   magnesium 
sulphate  and  potassium  chloride  are  also  given. 

MAGNESIUM    GHROMATE    MgCrO4.7H2O. 

100  grams  H2O  dissolve  72.3  grams  MgCrO4  at  18°,  or  100  grams 
solution  contain  42.0  grams.      Sp.  Gr.  =  1.422. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 

MAGNESIUM    POTASSIUM    CHROMATE    MgCrO4.K2CrO4.2H2O. 
100  grams  H2O  dissolve  28.2  grams  at  20°,  and  34.3  grams  at  60°. 

(Schweitzer.) 

MAGNESIUM    PLATINIC    CYANIDE    MgPt(CN)4. 
SOLUBILITY  IN  WATER. 

(Buxhoevden  and  Tamman  —  Z.  anorg.  Ch.  15,  319,  '97.) 


Gms.MgPt(CN)4 

Gms.  MgPt(CN)4 

t  °. 

per  100  Gms. 

Solid  Phase. 

t°. 

per  100  Gms. 

Solid  Phase. 

Solution. 

Solution  . 

-4-12 

24.90 

MgPt(CN)4.6.8-8.iH2O 

48.7 

40.89 

MgPt(CN)4.4H20 

o-5 

26.9 

"        (Red) 

55 

41-33 

" 

5-5 

28.65 

" 

58.1 

42.15 

" 

18.0 

32.46 

" 

69.0 

43-49 

'• 

36.6 

39-53 

" 

77.8 

44.90 

" 

45  -° 

4i-33 

« 

87.4 

45-52 

" 

46.2 

42  .0 

« 

90.0 

45-65 

«« 

42.2 

40.21 

MgPt(CN)4.4H2O 

93-o 

45-04 

•« 

46-3 

39.85 

"     (Bright  Green) 

96.4 

44-33 

MgPt(CN)4.2H2O 

100.  0 

44-o 

(White) 

MAGNESIUM    FLUORIDE    MgF2. 
One  liter  of  water  dissolves  0.076  gram  MgF2  at  18°  by  conductivity 

method.  (Kohlrausch  —  Z.  physik.  Ch.  50,  356,' 04- '05. 


MAGNESIUM    HYDROXIDE    Mg(OH)2. 
One  liter  of  water  dissolves  0.008  —  0.009  gm-  Mg(OH)2  at   18°  by 

Conductivity  method.  (Dupre  and  Brutus  — Z.  angew.  Ch.  16,  55,  '03.) 

SOLUBILITY  OF  MAGNESIUM  OXIDE  IN  AQUEOUS  SOLUTIONS  CONTAINING 
SODIUM  CHLORIDE  AND  SODIUM  HYDROXIDE. 

(Maigret  —  Bull.  soc.  chim.  33,  631,  '05.) 

Grams  MgO  per  Liter  Solution  with  Added: 


Gms.  NaCl 
per  Liter. 

125 
I4O 

160 


0.8  g.  NaOH 
per  Liter. 

O.O7 
0.045 

none 


4.0  g.  NaOH 
per  Liter. 

0.03 


none 


MAGNESIUM    HYDROXIDE      182 

SOLUBILITY  OF  MAGNESIUM  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OP 
AMMONIUM  CHLORIDE  AND  OF  AMMONIUM  NITRATE  AT  29°. 

(Herz  and  Muhs  —  Z.  anorg.  Ch.  38,  140,  '04.) 

NOTE.  —  Pure  Mg(OH)2  was  prepared  and  an  excess  shaken  with 
solutions  of  ammonium  chloride  and  of  ammonium  nitrate  of  different 
concentrations. 


Concentration  of 

Acm  Kequirea 
for  Liberated 

Normality  of: 

Grams  per  Liter. 

(Normal.) 

(Normal.)  CC< 

'Mg(OH)2.    NH4C1'. 

Mg(OH)2.    NH4C1. 

.  7         (NH4C1) 

0.09835 

0.156      0.388 

4.55     20.86 

o  .  466 

O.IIOS 

0-loS      0.250 

3-!5     *3-39 

o-35 

0.09835 

0.089      0.172 

2.60      9.21 

0-233 

O.IIOS 

0.0638  0.106 

1.86      5.67 

O.IIOS 

0.049     0.0771 

i-43       4-i3 

0.35      (NH4N03) 

O.IIOS 

0.0833    O.l834(NH4NO3)2  .43       14.69 

0.175 

O.IIOS 

0.0495  0.076 

"      i-45       6.09 

MAGNESIUM    IODATE    Mg(IO3)2. 

SOLUBILITY  IN  WATER. 

(Mylius  and  Funk  —  Ber.  30,  1722,  '97;  Wiss.  Abh.  p.  t.  Reichanstalt  3,  446,  'oo.) 


Gms. 

Mols. 

Gms. 

Mols. 

to           Mg(I03)2 
per  TOO 

Mg(I03)2            Solid 
per  loo  Mols.        Phase. 

t       • 

Mg(I03)2    Mg(I03)2            Solid 
per  100     per  too  Mols.        Phase. 

Gms.  Solution. 

H20. 

Gms.  Solution. 

H20. 

0 

3 

.1 

O 

.15      Mg(I03)2.ioH20 

0 

6 

.8 

o-34 

Mg(I03)2.4H20 

20 

10 

.2 

O 

•55 

10 

6 

•4 

0.30 

" 

30 

17 

•4 

I 

.01 

18 

7 

.6 

0.40 

«• 

35 

21 

9 

I 

•35 

20 

7 

•7 

0.40 

" 

67. 

5 

10 

.0 

35 

8 

•9 

0.47 

" 

63 

12 

.6 

0.69 

" 

100 

J9 

•3 

i  .13 

" 

Sp.  Gr.  of  solution  sat.  at  18°=  1.078. 


MAGNESIUM    IODIDE    MgI2. 

SOLUBILITY  IN  WATER. 

(Menschutkin  —  Chem.  Centrb.  77,  I,  646,  '06;  at  18°,  Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 


O 
10 

18 

20 

25 
30 
40 

45 


Solid 
Phase. 

MgI2.8H2O 


Gms.  MgI2  per 
100  Grams  Solution. 

5O.O 

53.0  (59.7  M.andF.) 

53-4 

54-4 

55-4 
57-8 
59-9 

Density  of  saturated  solution  at  18°=  1.909.     (M.andF.) 


to      Grams  MgI2  per           Solid 
'  100  Grams  Solution.      Phase. 

50 

6l.6 

MgI2.6H20 

70 

61.85 

" 

90 

62  .  I 

M 

110 

62.25 

" 

I4O 

62-5 

" 

1  60 

63.0 

" 

200 

64.1 

" 

183  MAGNESIUM  IODIDE 

SOLUBILITY    OF   MAGNESIUM   IODIDE  ALCOHOL  COMPOUNDS    IN   THE 
CORRESPONDING  ALCOHOLS. 

(Menschutkin  —  Chem.  Centrb.  77,  I,  335,  '06.) 

Results  expressed  in  molecular  per  cent. 

«.0     MgI2.6CH3OH  MgI2.6C2H5OH  .0     MgI2.6CH3OH     MgI2.6C2H8OH   ' 

*•       inCH3OH.      in  C2H6OH.  *'        in  CH3OH.         inC2HfiOH. 

o  6.3  2.3  ioo  10.5  19.7 

10  6.6  3.1  120  ii. 8  28.2 

20  7.0  4.0  140  13.4  53-6 

40  7.8  6.2  160  15.7  80.3(145°) 

60  8.6  9.3  180  18.7  100.0(146.5°) 

80  9.5  13.5  200  23.1 


SOLUBILITY  OF  MAGNESIUM  IODIDE  Di  ETHERATE  (MgI2.2C4Hi0O)  IN 

ETHYL  ETHER. 

(Menschutkin  —  Z.  anorg.  Ch.  49,  46,  '06.) 

Synthetic  Method  used,  see  Results  in  the  Critical 

page  9.  Vicinity. 

0  Grams  per  ioo  Gms.  Solution.  Gms.  per  ioo  Cms.  ScJution. 

MgI2.      MgI2.2C4H10O.  '  MgI2.        MgI2.2C4H,0O. 

5-4  i-45  2.2  37-3  *9-4  29.3 

ii. 8  2.43  3.7  38.5  22.45  34-4 

J5-6  3-46  5.3  38-5  26.07  39-9 

18.1  5.4  8.3  38.5  29.8  45.7 
20.4  7.55  ii. 6  38  32.8  50.3 

22.2  11.28  17.3 

Two  liquid  phases  appear  near  the  melting  point  of  the  magnesium 
iodide  di  etherate.  The  lower  may  be  considered  as  a  solution  of  ether 
in  di  etherate,  and  the  upper  as  a  solution  of  the  lower  layer  in  ether. 
The  critical  temperature  is  38.5°. 

Lower  Layer.  Upper  Layer. 

0  Gms.  per  ioo  Gms.  Solution.  Gms.  per  ioo  Gms.  Solution 

MgI2.          MgI2.2C4H100.  '  '  MgI2.  MgI2.2C4H100.  " 

14-8  35.5  54.4  18.6  13.57  20.8 

20.0  35.8  54.8  23.2  14.4  22.1 

28.4  35.5  54.4  24.4  14-6  22-4 

33  35-7  54-7  32-4  i5-82  24.2 

35  35-3  54-i 

The  solubility  of  double  compounds  of  magnesium  iodide  and 
alkyl  esters  in  the  corresponding  acetates  is  given  by  Menschutkin  — 
Chem.  Centrb.  77,  I,  647,  '06.  For  the  solubility  of  magnesium  iodide 
hexa  acetic  acid  compound  in  anhydrous  acetic  acid  solutions,  see  Chem. 
Centrb.  77,  II,  1482,  '06. 


MAGNESIUM    NITRATE  184 

MAGNESIUM    NITEATE   Mg(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  437,  *oo.) 

Gms.  Mols.                                                         Gms.                Mols. 

Mg(NO3)2  Mg(NO3)2              Solid                           Mg(NO3)2       Mg(NO3)2           Solid 

t°.     per  ioo  Gms.  per  ioo  Mols.           Phase.  t°.     per  ioo  Gms.   per  ioo  Mols.        Phase. 

Solution.  H2O.                                                       Solution.              H2O. 

—  23         35-44  6.6         Mg(N03)2.9H20  40         45-87            10.3       Mg(NO3)2.6H2O 

—  20         36.19  7-0  80         53-69            14.6 

— 18      38.03         7.4  90       57.81         16.7 

— 18         38.03  7.37      Mg(N03)2.6H20        89         63.14  20-9J 

-4-539-50        7-92  "  77-5  65-67        23.2  V* 

o      39-96        8.08  67      67.55        25-1  ) 

-f-l8         42-33  8.9  *  Reverse  curve- 

Sp.  Gr.  of  solution  saturated  at  18°  =  1.384. 
MAGNESIUM    OXALATE    Mg.C2O4.2H2O. 
One  liter  of  water  dissolves  0.3  gram  MgC2O4  at    18°  (conductivity 

method).  (Kohlrausch  — Z.  physik.  Ch.  50,  356,  '05.) 

MAGNESIUM    (Hypo)    PHOSPHATE    Mg2P2O6.i2H2O. 
One  liter  of  water  dissolves  0.066  gram  hypophosphate. 

(Salzer  —  Liebig's  Ann.  232,  114,  '86.) 

One   liter   of   water   dissolves    5.0    grams   magnesium   hydrogen 
hypophosphate  MgH2P2O6.4H2O.  (Salzer.) 

MAGNESIUM    SALICYLATE    Mg(C7H5O3)2.4H2O. 

One  liter  of  saturated  solution  contains  8.015  grams  of  the  salt. 

(Barthe  —  Bull.  soc.  chim.  [3]  n,  519,  '94.) 

MAGNESIUM    FLUOSILICATE    MgSiF6.6H2O. 

One  liter  of  water  dissolves  652  grams  of  the  salt  at  17.5°.     Sp.  Gr. 

Of  Solution  =   1.235.  (Stolba  —  Chem.  Centrb.  578,  '77 •) 

MAGNESIUM    SULPHATE    MgSO4. 

SOLUBILITY  IN  WATER. 

(Mulder;  Tilden  —  J.  Ch.  Soc.  45,  409,  '84;  Etard  —  Com pt.  rend,  106,  741,  '88.) 

Etard' s  results  for  the  lower  temperatures  are  somewhat  low. 
Mulder's  and  Til  den's  results  agree  very  well. 

to       Gms.  MgSOj  per  ioo  Gms.  Solid  to        Gms.  MgSO4  per  ioo  Gms.          Solid 

Solution.         Water.  Phase.  Solution.  Water.  Phase. 


O  21.2  26.9       MgSO4.7H2O  50  33-5  50-3 

10        24.0        31.5  ••  60        35.5        55.0 

20  26.5  36.2  70  37.5  59.6 

25  28.2  38.5  80  39.1  64.2 

30  29-0  40.9  "  90  40.7  68.9 

40        31.2         45.6  "  ioo         42.5         73.8 

no        45-5        83.6 

For  temperatures  between  123°  and  190°,  grams  MgSO4  per  ioo  grams 
solution  =  48.5  -0.4403  t.  (Etard). 

For  densities  of  aqueous  solutions  of  MgSO,,  see  Barnes  and  Scott— 
J.  Physic.  Ch.  2,  542,  '98. 


185  MAGNESIUM    SULPHATE 

SOLUBILITY  OF  MAGNESIUM  SULPHATE  IN  METHYL  AND  ETHYL 

ALCOHOLS. 

(de  Bruyn  —  Rec.  trav.  chim.  n,  112,  '92.) 
Solvent.          t°.        Per  100  Gms.  Solvent.  Solvent.  t°.      Per  100  Cms.  Solvent. 

Abs.  CH3OH     18       1.18  gms.  MgS04  93%  Methyl  Ale.     17     9.7  gms.MgSO4.7H2O 

17     41-0       "     MgS04.7H20    50%       "         «       3-4     4.1      « 
"  3-4    29.0      "  Abs.  C2H5OH  3     1.3     "  " 

SOLUBILITY  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Schiff  —  Liebig's  Ann.  118,  365,  '61.) 

Wt.  per  cent  Alcohol  10  20  40 

G.  MgSO4.yH2O  per  100  gms.  solvent        64.7         27  .1         i  .65 

SOLUBILITY  OF  MAGNESIUM  SULPHATE  IN  SATURATED  SUGAR  SOLUTION 

AT    31.25°. 
(Kohler  —  Z.  Ver.  Zuckerind.  47,  447,  '97.) 

ioo  grams  saturated  aqueous  solution  contain  46.52  grams  sugar -f 
14.0  grams  MgSO4. 

ioo  grams  water  dissolve  119.6  grams  sugar  +  36.0  grams  MgSO4. 


MAGNESIUM    POTASSIUM    SULPHATE    MgK2(SO4)2.6H2O. 
SOLUBILITY  IN  WATER. 

(Tobler —  Liebig's  Ann.  95,  193,  '55.) 

t°.-o°          20°       30°        45°        60°        75° 
Gms.  MgK2(S04)2 
per  ioo  gms.  H2O     14.1       25.0      30.4      40.5       50.2       59.8 

MAGNESIUM    SULPHITE    MgSO3.6H2O. 

ioo  grams  cold  water  dissolve  1.25  grams  sulphite;  ioo  grams  boil- 
ing water  dissolve  0.83  gram. 

(Hager  —  Chem.  Centrb.  135,  '75.) 

MALONIC    ACID    CH2(COOH)2. 

SOLUBILITY  IN  WATER. 

(Klobbie  —  Z.  physik.  Chem.  24,  622,  '97;  Miczynski  —  Monatsh.  Ch.  7,  259,  '86;  Henry  —  Compt.  rend 
99,  1157,  '84;  Lamouroux  —  Ibid.  128,  '998,  '99.) 

Grams  CH2(COOH)2  per  ioo  Grams  CH2(COOH)2  per  ioo 


I    . 

Gms.  Solution.* 

cc.  Solution  (L.). 

Gms.  Solution.* 

cc.  Solution  (L.; 

o 

52.0 

61  .0 

So 

71.0 

93-o 

10 

56.5 

67.0 

60 

74-5 

100.0 

20 

60.5 

73-o 

70 

106.0 

25 

62  .2 

76-3 

80 

82.0 

30 

64.0 

80.0 

IOO 

89.0 

40 

68.0 

86.5 

132 

(m.  pt.)  loo-o 

*  Average  curve  from  results  of  K.,  M.,  and  H. 


MALONIC    ACID 


186 


SOLUBILITY  OF  MALONIC  ACID  IN  ETHER. 

(Klobbie.) 


k°. 

Gms.  CH2(COOH)2 
per  ioo  Gms. 
Solution. 

f. 

Gms.  CH2(COOH)2 
per  ioo  Gms. 
Solution. 

o 
10 

7-74 

30 
80 

10-5 

33-o 

20 

9.00 

90 

39-o 

25 

9-7 

Gms.  CH2(COOH)2 
t  °.  per  ioo  Gms. 

Solution. 

IOO  46.0 

no  56-0 

120  70.0 

132  (m.  pt.)      100.0 


ioo  grams  saturated  solution  of  malonic  acid  in  pyridine  contain 
14.6  grams  at  26°. 

(Holty  — J.  Physic.  Ch.  9,  764,  '05.) 

SOLUBILITY  OF  SUBSTITUTED  MALONIC  ACIDS  IN  WATER. 

(Lamouroux.) 
Grams  per  ioo  cc.  Saturated  Aqueous  Solution. 


t°. 

r 

Methyl 

Ethyl 

n  Propyl 

n  Butyl 

Iso  Amyl 

Malonic 

Malonic 

Malonic 

Malonic 

Malonic 

Malonic 

Acid. 

Acid. 

Acid. 

Acid. 

Acid. 

Acid. 

0 

61.1 

44-3 

52.8 

45-6 

ii.  6 

38.5 

15 

70.2 

58-5 

63.6 

60.  1 

30-4 

51-8 

25 

76.3 

67.9 

71.2 

70.0 

43-8 

79-3 

30 

92.6 

9r-5 

90.8 

94.4 

79-3 

83-4 

MANGANESE    BORATE   MnH4(BO3)2H2O. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SALT  SOLUTIONS. 

(Hartley  and  Ramage  —  J.  Ch.  Soc.  63,  137,  '93.) 

Grams  MnH4(BO3)2  per  Liter  in  Solutions  of: 


t°. 

H2O  + 

Na2S04 

Na2S04 

NaCl 

CaCl2 

trace 

(0.2  Gms 

(20  Gms. 

(20  Gms. 

(20  Gms. 

Na2SO4. 

per  Liter).         per  Liter). 

per  Liter). 

per  Liter). 

14 

0-94 

I  .7 

18 

0-77 

I-3I 

2  .91 

40 

0.50 

0.69 

(52°)    0.65 

2.44 

60 

0.36 

O-6o 

2.25 

80 

0.08 

0.12 

0.29 

MANGANESE    BROMIDE    MnBr2.4H2O. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  537,  '94.) 


t°. 

Gms.  MnBr2 
per  ioo  Gms. 
Solution. 

Solid 
Phase. 

t°. 

Gms.  MnBr2 
per-ioo  Gms. 
Solution. 

Solid 
Phase. 

—  20 

52-3 

MnBr2.4H2O 

40 

62.8 

MnBr2.4H2O 

—  10 

54-2 

u 

50 

64-5 

" 

0 

56.0 

" 

60 

66.3 

« 

10 

57-6 

" 

70 

68.0 

» 

20 

59-5 

(1 

80 

69.2 

MnBr.2H2O 

2$ 

60.2 

II 

90 

69-3 

.• 

30 

61.1 

M 

IOO 

69-5 

•« 

i87 


MANGANESE    CHLORIDE 


MANGANESE    CHLORIDE    MnCl2.4H2O. 

SOLUBILITY  IN  WATER. 

(Etard;  Dawson  and  Williams  —  Z.  physik.  Chem.  31,  63,  '99-) 

Mols.  MnCJ2 
per  100  Mols.  H2O. 


,.  o                 Sp.  Gr.  of      G 

rams  MnCJ2  per  100  Gram 

Solutions. 

Water 

Solution. 

—  20 

53-8 

35-o 

—  10 

58-7 

37-o 

O 

63-4 

38-8 

+  10 

68.1 

40-5 

20 

73-9 

42-5 

25 

.4991 

77.18 

43-55 

30 

•5049 

80.71 

44-68 

40 

•5348 

88.59 

46.96 

50 

•5744 

98.15 

49-53 

57-65 

.6097 

105.4 

5J-33 

60 

.6108 

108.6 

52.06 

70 

.6134 

no.  6 

52-52 

80 

112.7 

52.98 

90 

114.1 

53-2 

100 

ii5-3 

53-5 

1  20 

118.8 

54-3 

140 

iiQ-5 

55-o 

II.OS 

IJ-55 

12  .69 
14.05 
15  .IO 

J5-55 
15-85 
16.14 


Solid 
Phase. 


MnCl2.2H2O 


One  liter  of  water  dissolves  87.0  grams  MnCl2.    One  liter  of  sat.  HC1 


dissolves  19.0  grams  MnCl2  at  12 


(Ditte  —  Compt.  rend.  92,  242,  '81.) 


MANGANESE    FLUO    SILICATE    MnSiF6.6H2O. 

100  grams  H2O  dissolve  140  grams  salt  at  17.5°.    Sp.  Gr.  of  solution 

=    1.448.  (Stolba  — Chem.  Centrb.  292,  '83.) 


MANGANESE    NITRATE    Mn(NO3)2.6H2O. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  438,  'oo.) 


0 

Gms. 
Mn(NO3)2 

Mols. 
Mn(NO3)2                Solid 

t  °. 

Gms. 
Mn(N03)2 

Mols. 
Mn(N03)2              Solid 

par  100 
Gms.  Sol. 

per  100                 Phase. 
Mols.  H2O. 

per  TOO 
Gms.  Sol. 

per  TOO                  Phase. 
Mo]s.H2O. 

-29 

42.29 

7 

.37      Mn(NO3)2.6H2O. 

18 

57 

•33 

13 

.5 

Mn(NO3)2.6H2O. 

-26 

43-15 

7 

•63 

25 

62 

•37 

16 

•7 

» 

—  21 

44-3° 

8 

•  O 

27 

65 

.66 

J9 

.2 

Mn(NO3)2-3H2O. 

-16 

45-52 

8 

•4 

29 

66 

•99 

2O 

4 

" 

-  5 

48.88 

9 

.61                «« 

67 

•38 

20-7 

o 

50-49 

10 

.2 

34 

71 

•31 

24 

9 

" 

+  11 

54-50 

12 

.0 

35-5 

76 

.82 

33 

3 

•• 

Sp.  Gr.  of  solution  saturated  at  18°  =  1.624. 


MANGANESE    (Hypo)    PHOSPHITE    Mn(PH2O2)2H2O. 

100  grams  H2O  dissolve  15.15  grams  salt  at  25°,  and  16.6  grams  at 
b.  pt. 


MANGANESE    SULPHATE 


188 


MANGANESE    SULPHATE    MnSO4>5H2O. 

SOLUBILITY  IN  WATER. 

(Cottrell  —  J.  Physic.  Ch.  4,  651,  '01;  Richards  and  Fraprie  —  Am.  Ch.  J.  26,  77,  '01.  The  results 
of  Linebarger  —  Am.  Ch.  J.  15,  225,  '93,  were  shown  to  be  incorrect  by  Cottrell,  and  this  conclusion 
was  confirmed  by  R.  and  F.) 


Grams  MnSO4  per 
4°.                 loo  Gms. 

'    Water. 

Solution. 

10 

47 

.96 

32 

.40 

O 

53 

•23 

34 

•73 

5 

56 

.24 

35 

•99 

9 

59 

•33 

37 

.24 

12 

61 

•77 

38 

.19 

14-3 

63 

•93 

39 

.00 

5 

58 

.06 

36 

.69 

9 

59 

.19 

37 

.18 

15 

61 

.08 

37 

.91 

25 

64 

•78 

39 

67 

•76 

40 

•38 

35-5 

71 

.61 

4i 

•74 

Solid  Phase. 


MnSO4.7H2O 


MnSO4.sH2O 


Grams  MnSO4  per 
t°.                    100  Gms. 

Water. 

Solution. 

16 

63.94 

38-99 

18.5 

64.19 

39.10 

25 

65  -32 

39-53 

30 

66.44 

39-93 

39-9 

68.81 

40.77 

49-9 

72.63 

42.08 

41.4 

60.87 

37-84 

5° 

58.17 

36.76 

60 

55-o 

35-49 

70 

52.0 

34-22 

80 

48.0 

32-43 

90 

42-5 

29.83 

100 

32.0 

24.24 

Solid  Phase 


MnSO4.4H2O 


MnSO4.H2O 


SOLUBILITY   OF   MANGANESE    SULPHATE,    COPPER   SULPHATE  MIXED 
CRYSTALS  IN  WATER  AT  18°. 

(Stortenbecker  —  Z.  physik.  Chem.  34,  112,  'oo.) 


Mols.  per  100  Mols.        Mol.  per  cent 
H8O.  Cu  in  : 

'Cu.  Mn.          Solution.     Crystals. 

Solid  Phase,  CuMnSO4.sH2O,  Triclinic. 

2.282     o 


2.23      0-44 


i-54      3-76 


4.70 


[I  .06         5.58 


Mols.  per  100  Mols. 
H20. 


Mol.  per  cent 
Cu  in: 


100 

100 

[0 

73 

6-37 

90 

•5 

. 

. 

83 

•5 

. 

O 

34 

7- 

03 

74 

.1 

97 

•3 

. 

. 

57 

•7 

95 

.1 

. 

7- 

37 

31 

.0 

81 

•3 

Solid 

Phase 

.  Cu 

29 

.0 

26 

21 

.1 
.8 

70 

•4 

[i- 

,06 

5'. 

58 

21 

2O 

.2 
•  O 

42 
34 

.6 
•4 

[a. 

73 

6. 

37 

15 

I3 

9 
9 

22 
15 

•9] 

.2* 

• 

±8 

Cu.  Mn.          Solution.     Crystals. 

Solid  Phase,  CuMnSO4.sH2O.  Triclinic. 

10.27       10.5] 

5.0        4-9 
4 . 60 


2.31 
o.o 


2.15 

O-O 


20-4         28.2* 

15-9 
12  .45 

10.27 


o.o 


23.5] 
20.8 

16.0] 
5.8* 
o.o 


*  Indicates  meta  stabil  points. 


CuMnSO4.5H2O  =  100-90.8  and  2.11-0  mol.  percent  Cu. 
CuMnSO4>7H2O  =  37.8-4.92  mol.  per  cent  Cu. 


SOLUBILITY  OP  MANGANESE  SULPHATE  IN  GLYCOL. 
100  grams  saturated  solution  contain   0.5  gram  MnSO4. 

fde  Coninck  —  Bui.  acad  roy.  Belgique,  359,  '05.) 


i89  MANGANESE    SULPHATE 

SOLUBILITY  OF  MANGANESE  SULPHATE  IN  AQUEOUS  ETHYL  AND 
PROPYL  ALCOHOL  SOLUTIONS  AT  20°. 

(Linebarger  — Am.  Ch.  J.  14,  380,  '92;     Snell  — J.  Physic.  Ch.  2,  474,  '98.) 

Cone,  of  Alcohol       Cms.  MnSO4  per  100  Cms.  Aq.      Cone,  of  Alcohol     Gms.MnSO4  per  looGms.  Aq. 
in  Wt.  per  cent.        Ethyl  Ale.  Propyl  Ale!       in  Wt.  per  cent.      Ethyl  Ale.       '      Propyl  Ale.' 

34  9-5  6.0  44  3-3  *-9 

36  7-2  4.6  48  2.2  1.4 

38  S-8  3-5  52  i-4  LI 

40  4.7  2.8 

MANGANESE    POTASSIUM    VANADATE    MnKV5O14.8H2O. 
100  grains  H2O  dissolve  1.7  grams  salt  at  18°. 

(Radan  —  Liebig's  Ann.  251,  129,  '89.) 

MANNITE    C6H8(OH)6. 

SOLUBILITY  IN  WATER. 

(Campetti  —  Abs.  in  Z.  physik.  Chem.  41,  109,  '02.) 

Grams  CeHgCOH^  per  100  Grams. 
'  Water.  Solution. ' 

10  T3-94  12.78 

15  16.18  14.63 

20  18.98  16.86 

100  grams  of  saturated  solution  of  mannite  in  Pyridine  contain  0.47 
gram  C6H8(OH)6  at  26°.  (Hoity  — j.  Physic.  Ch.  9, 764,  '05.) 

MANNITOL    C6H8(OH)6. 

SOLUBILITY  IN  WATER. 

(Findlay  — J.  Ch.  Soc.  81,  1219,  '02.) 

Gms.  G.M.                                                                     Gms.  G.  M. 

+  o      Wt.  of  i  cc.           Mannitol  Mannitol  .  0      Wt.  of  i  cc.                     Mannitol  Mannitol 

in  Grams.               perioo  per  100                     '       in  Grams.                        per  100  per  100 

Gms.H2O.  G.M.H2O.                                                            Gms.H2O.  G.M.H2O. 

o    1.044  7-59        o-75  50     1-099  (47-7°)     47-Qi        4-65 

10       ...  11-63         I<IS  60       •••  60. 01        5-94 

15     1.05  14-38        1-42  70     1-148(68°)        74.50        7.35 

20       ...  J7-71        *-75  80       ...  9l-5          9-O4 

25       ...  2I-39        2. ii  90     1.207  (85-9°)    no. 8        10.96 

30     i. 076(31. i°)25-4o         2.51          100       ...  133-1         13.17 

40       ...  35.40        3.50 

NOTE.  —  In  the  original  paper  the  author  writes,  "  grams  of  sub- 
stance in  100  grams  of  solvent  (percentage  solubility) "  and  "  moles 
of  substance  in  100  mols  of  solvent  (percentage  molar  solubility),"  thus 
implying  equivalence  of  the  terms  and  giving  rise  to  uncertainty  as  to 
which  is  really  intended. 

MERCURY   BROMIDE    (ic)    HgBr2.      SOLUBILITY  IN  WATER. 

*"•  ^(MS:  Authority. 

Q  I    06  (Lassaigne  —  J.  chim.  med.  12,  177, '76.) 

2e  Q.6l  (Sherrill  — Z.  physik.  Ch.  43,  727,  '03.) 

100  20-25  (Lassaigne.) 


MERCURY    BROMIDE  190 

SOLUBILITY  OP  MERCURIC  BROMIDE  ORGANIC  SOLVENTS. 
In  Carbon  Bisulphide.  In  Other  Solvents   at  i8°-2o°. 

(Arctowski  —  Z.  anorg.  Ch.  6,  267,  '94.)  (Sulc.  —  Ibid.  25,  401,  'oo.) 

Gms.HgBr2  Gms.  HgBr2  Gms.  HgBr2 

te.       per  100  Gms.        t°.       per  100  Gms.  Solvent.  Formula.     periooGms. 

Solution.  Solution.  Solvent. 

—  io        0.049         I5        0.140    Chloroform  CHC13      0.126 

—  5        0.068        20        0.187     Bromoform  CHBr3      0.679 
o        0.087         25        0.232     Tetra  Chlor  Methane    CC14         0.003 

-f  5        0.105        30        0.274    Ethyl  Bromide  C2H5Br     2.31 

io        0.122  Ethylene Di Bromide     C2H4Br2   2.34 

Mercurous  bromide  Hg2Br2.    One  liter  of  saturated  aqueous  solution 
contains  0.000039  gram  Hg2Br2  at  25°.  (Shemii) 

MERCURY    CHLORIDE    (ic)    HgCl2. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  563,  '94;  at  25°,  Foote  and  Levy  —  Am.  Ch.  J.  35,  238,  '06;  at  room 
temp.     Rohland  —  Z.  anorg.  Ch.   18,  328'  '98;  see  also  Poggiale  —  Ann.  chim.  phys.  [3]  8,  468,  '43.) 


to         Gms.  HgCl2  per 
loo  Gms.  Solution. 

AO         Gms.  HgCl2  per 
100  Gms.  Solution, 

+  o           Gms.  HgG2  per 
zoo  Gms.  Solution. 

0 

3-5 

30 

7-2 

IOO 

38.0 

10 

4-5 

40 

9-3 

120 

59-o 

2O 

5.4(6.88,R. 

60 

14.0 

I4O 

77.0 

25 

6.9  (F.  and  L.) 

80 

23.1 

ISO 

78.5 

SOLUBILITY    OF    MERCURIC    CHLORIDE    IN    AQUEOUS    SOLUTIONS    OF 

SODIUM  CHLORIDE. 

(Homeyer  and  Ritsert  —  Pharm.  Ztg.  33,  738,  '88.) 


Per  cent  Concentration  Gms'  H*CI2  P"  I0°  Gms'  NaC1  Sohltion  at; 

of  NaCl  Solutions. 

0-5 
I  .O 

5-o 

IO-O 

25.0 

26.0  (saturated)  128 

SOLUBILITY    OF    MERCURIC    CHLORIDE    IN    AQUEOUS    SOLUTIONS    OF 

HYDROCHLORIC  ACID  AT: 
o°.  20-25°  (?)• 

(Engel  —  Ann.  chim.  phys.  [6]  17,  362,  '89.)  (Ditte  —  Ibid.  [5]  22,  551,  '81.) 


15° 

65° 

100° 

10 

13 

44 

14 

18 

48 

30 

36 

64 

58 

68 

no 

1  2O 

142 

196 

128 

152 

208 

f.  Mols.  per 
HC1. 

IOO  CC.  Sol. 

*HgCl. 

Gms.  per 
HC1. 

IOO  CC.  Sol. 

HgCl2. 

Sp.  Gr.  of 
Solutions. 

jfarts  nu 

per  zoo 
Parts  H2O. 

raits  Hg( 

per  loo 
Parts  Solu 

4-3 

9-7 

i-57 

I3.II 

I.II7 

o.o 

6.8 

9-9 

19.8 

3.61 

18.04 

1.238 

5-6 

46.8 

17.8 

35-5 

6.49 

32-44 

1.427 

10.  1 

73-7 

26.9 

55-6 

9.81 

49.04 

1.665 

i3.8 

87.8 

32-25 

68.9 

n  .76 

58.80 

1.811 

21  .1 

127.4 

34-25 

72.4 

12.48 

62.40 

1.874 

31.0 

141.9 

4i-5 

85  5 

J5-I3 

75-65 

2  .023 

5O.O 

148.0 

48.1 

88  6 

17-54 

87.70 

2.066 

68.0 

154.0 

70.9 

95-7 

25.84 

129.20 

2.198 

IQI  MERCURIC     CHLORIDE 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  AND  MERCURIC  CHLORIDE  IN 

WATER  AT  25°. 

(Foote  and  Levy  —  Am.  Ch.  J.  35,  239,  '06.) 


Gms.  per  100  Gms.  Solution.     Gms.  per  too  Gms.  Undissolved  Residue. 


NaCl. 


HgCl2. 


NaCl. 


HgCl2. 


H20. 


Solid 
Phase. 


26  .  5          none 
18.66        51.35 
18.71        51-32 
18.64        51-42 
18.87        5J-26 

14-97        57-74 
14.03        59.69 
13.25        62.16 
13.17        62.59 
12.97        62.50 
13.14        62.48 
13.15        62.55 

Two  determinations  made 

IOO 

16^8 
16.36 

16.16 
15.96 

at  10.3°  gave 

none 

16-39 
21.98 
65.42 

74-iS 

74.21 
74.70 
74.76 
78.20 
88.64 
90.83 

none 

:::, 

9-44 
9-43 
9.14 
9.28  , 

NaCl 

NaCl  and 
NaCl.HgCJ2.2H20 

D6uble  Salt 
NaCl.HgCl2.2H20 
Calc.  Comp.  =  16.01%  NaCl 
74-14%  HgCl.9.85%  H20 

NaCl.HgCl2.2H20 
and  HgCl2 

19.46 

46.49 

67.46 

29.19 

3-35 

19.48 

46.50 

22.83 

68.85 

8-32 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  AND  MERCURIC  CHLORIDES 
IN  WATER  AT  25°. 

(Foote  and  Levy.) 


Solid 
Phase. 


Composition  of  Solution. 
Grams  per  100  Grams 
Solution. 

Percentage  Composition 
of  Undissolved 
Residue 

'    KC1. 

HgCl2. 

KCl. 

HgCl2. 

H2O. 

26.46 

none 

IOO 

none 

26.24 

15.04 

3-63 

26.43 

15  .02 

26.15 

26.33 

15.02 

52.01 

26-33 

14.92 

61  .04 

23-74 

18.91 

34.61 

61.66 

3-73 

22.36 

21.39 

34-77 

62  .02 

3-2i 

21-39 

23.88 

34-05 

61-84 

3-35 

20.32 

27  .62 

65.24 

2O.26 

27.38 

73-98 

I7-85 

25-34 

21.89 

75  -io 

3.01 

9.26 

18.95 

21  -O2 

73-36 

5.62 

7.80 

19.56 

20.76 

73.06 

6.18 

6.84 

22.81 

20-75 

74-54 

4.71 

6.66 

24.32 

20-54 

73-99 

5-47 

6.52 

25-I3 

76.46 

6.64 

25  -16 

.  .  . 

80.60 

6.27 

25  .11 

12  .09 

83.20 

4.71 

5-77 

24-73 

11.87 

83.18 

4-95 

4.68 

24-75 

84.46 

4.66 

25-*7 

93.68 

4.69 

24.82 

98.50 

none 

6.90 

none 

IOO-OO 

none 

KCl 


KC1  and 
2KCl.HgCl3.H2O 


2KCl.HgCl2.H2p 
Calc.  Composition 
34-05%  KCl,  6i.84%HgCl2, 
4.11%  H20 

2KCl.HgCI2.H20  and 
KCl.HgCl2.H20 


KCl.HgCl2.H2p 
Calc.  Composition 
20.52%KC1,  74-53%  HgCl2) 
5-47%  H20 


KCl.HgCl2.HoO  and 
KC1.2HgCl2.2H2O 

KC1.2HgCl2.2H20 
Calc.  Composition 
1 1 .43%  KCl,  83 .05%  HgCl2.5 -52%  H20 


KC1.2HgCl2.2H2O  and  HgCl2 
HgCl2 


MERCURIC    CHLORIDE 


192 


SOLUBILITY  OF  MIXTURES  OF  RUBIDIUM  AND  MERCURIC   CHLORIDES 

IN  WATER  AT  25°. 

(Foote  and  Levy,) 


Composition  of  Solution. 
Grams  per  100  Grams. 

Percentage  Composition 
of  Undissolved  Residue.                          Solid 

Solution. 

Phase. 

'  RbCl. 

HgCl2.   " 

RbCl. 

HgCl2. 

H20. 

48-57 

none 

IOO.O 

none 

none       RbCl 

46.76 

9.18 

88.04 

ii  .24 

0.72  ' 

47-54 
47-55 

9-49 
9-39 

60.33 
56-59 

37-51 
40-75 

2.16 
2.66 

RbCl  and  2RbCl.HgCl2.H2O 

47-3 

9-47 

46.73 

49-38 

3-88  J 

47-65 
35-i6 

10-35 
19.58 

46.50 
45-98 

50.92 
50.80 

2-58 
3.22 

2RbCl.HgC]2.H2O  Calc.  Com- 
position 45  .55%  RbCl.si  .05% 
HgCl2.3.4%H20 

34-77 

19.94 

43-07 

52-44 

4-49 

2RbCl.HgCl2.H2Oand  3RbCl. 

34-76 

20.  10 

41  .10 

55-36 

3-54 

2HgCl2.2H2O 

30.27 

20.17 

39-07 

57-34 

3-59 

3RbCl.2HgCl?.2H2O 

29.20 
27.38 

2o-55 
20.63 

39-10 
38.67 

57-47 
57-40 

3-43  . 
3-93 

Calc.  Composition 
38.55%RbCl,      57.62%HgCl2. 
3.82%H20 

26.83 
27.09 

20.87 
20.97 

38.48 
31.40 

57-36 
64-35 

4.16 
4-25 

•    3RbC1.2HgCl2.2H2O  and 
RbCl.HgCl2.H20 

26.15 

20.58 

30-34 

65.48 

4.18 

23.81 

18.71 

30.87 

65.10 

4-03 

RbCl.HgCl2.H20 
Calc.  Composition 

18.10 

14.25 

29.87 

65.28 

4-85 

-    29.49%  RbCl,  66.11%  HgCl2, 

10.87 

10.42 

29-33 

66.15 

4-52  . 

4-40%H2O 

10.68 
10.  06 

10.56 
10.05 

28.59 
26.22 

67.99 

72.20 

3-42 
1-58 

RbCl.HgCl2.H2O  and  3RbCl 
4HgCl2.H20 

io.c6 

9.86 

25.28 

73-38 

0.84  , 

8.48 
8.46 

8.71 
8.80 

25-30 
25-44 

73-15 
73-67 

!-55 
0.89 

3RbCl-4HgCl2.H2O 
Calc.  Composition 
'    24.76%  RbCl,  74.oi%HgCl2, 

5.68 

8.70 

25-09 

73-46 

i-45 

i.23%H2O 

5.10 

8-33 

24.92 

73-93 

I-I5 

3-43 

8.25 

22.79 

75-72 

i-49 

3RbC1.4HgCl2.H2Oand  RbCl 
rHeClo 

3-38 

8.00 

12.68 

86.74 

0.58 

5-tlo^->*2 

2.98 
1.89 

7.71 
7.64 

8.40 
8.38 

91.24 
91.78 

1RbCl.SHgCl2 
Calc.  Composition 

1.50 

7-55 

8-30 

91.81 

8.  20%  RbCl,  9i.8%HgCl2 

I  .10 

7.21 

8.07 

91.58 

.  ' 

0.79 

7.16 

6.91 

93-15 

•  «  •      j     RbC1.5HgCl2  and  HgCl-, 

0.84 

7.42 

2.27 

97.09 

...      j 

none 

6.90 

none 

IOO.O 

HgCl2 

193  MERCURIC    CHLORIDE 

SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  METHYL,  ETHYL  PROPYL, 
n  BUTYL,  Iso  BUTYL  AND  ALLYL  ALCOHOLS. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  563,  '94.) 

NOTE.  —  For  the  solubility  in  Me,  Et,  and  propyl  alcohols  at  room 
temperature,  see  Rohland  —  Z.  anorg.  Ch.  18,  328,  '98;  at  8.5°,  20°  and 
38.2°,  see  Timofejew  —  Compt.  rend.  112,  1224,  '91;  in  Me  and  Et 
alcohols  at  25°,  see  de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '92.  The  deter- 
minations of  these  investigators  agree  well  with  those  of  Etard,  which 
are  given  below. 

Grams  HgG2  per  100  Grams  Saturated  Solution  in: 


I     . 

CHgOH. 

C2H5OH. 

C3H7OH.     CH3(CH2j3OH.  (CH3)2CHCH2OH. 

CH2.CH.CHj,OH. 

-30 

14-5 

15.0 

—  20 

20.1 

J5-7 

J3-5 

21  .O 

—  10 

I5.2 

26.5 

I6.S 

13-7 

.  .  . 

25-5 

0 

2O.  I 

29.8 

17.4 

14.0 

5-2 

30.0 

+  10 

26.3 

30.6 

18.0 

14-3 

6.0 

37-5 

20 

34-o 

32.0 

18.8 

14.6 

6.8 

46-5 

25 

40.0 

32-5 

19-5 

J5-5 

7-2 

30 

44-4 

33-7 

20.0 

16.5 

7-5 

40 

58.6 

35-6 

23.0 

19.6 

9-7 

60 

62.5 

41.2 

29.8 

26.5 

17.0 

.  .  . 

80 

66.0 

47-5 

36.8 

33-o 

24.9 

100 

70.1 

54-3 

43-8 

31  .7 

1  20 

73-5 

61.5 

50.6 

39-2 

78.5 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  ACETIC  ACID. 

(Etard.) 


t°. 

Gms. 
HgCl2  per 
100  Gms. 

f. 

Gms. 
HgCl2  per 
loo  Gms. 

t<>. 

Gms. 
HgCU  per 
loo  Gms. 

Solution. 

Solution. 

Solution. 

20 

2-5 

70 

8-5 

no 

I3.6 

30 

3-5 

80 

9-7 

1  20 

16.5 

40 

4-7 

90 

II  .0 

130 

20.7 

50 

6.0 

IOO 

12.4 

140 

25.2 

60 

7-2 

160 

34-8 

SOLUBILITY  OF  MERCURIC  CHLORIDE  AND  SODIUM  CHLORIDE  IN  ETHYL 

ACETATE  AT  40°. 

(Linebarger  —  Am.  Ch.  ].  16,  214,  '94.) 


Mols. 

per  loo  Mols. 

Gms.  . 

per  100  Gms. 

Gms.  per 

loo  Gms. 

Acetate. 

Acetate 

Solution. 

Solid 
Phase. 

NaCl. 

HgCl2. 

NaCl. 

HgCl2. 

NaCl. 

HgCl2: 

0.8 

12-9 

0.53 

39-7 

o-53 

28.4 

HgCl2 

2-3 

12-4 

i-53 

38-15 

27.61 

it 

4-3 

l6-4 

2-85 

5°  -44 

2.78 

33-54 

" 

9.1 

22.85 

6.05 

86.14 

5.60 

46.28 

M 

18.5 

34-9 

12.29 

107.4 

10.95 

51.76 

II 

20.  o 

40.0 

13.29 

123.0 

n-73 

55-18 

HgCl2  +  NaCl 

The  double  salt  (HgCl2)2.NaCl  is  formed  under  proper  conditions. 


MERCURIC    CHLORIDE 


194 


SOLUBILITY    OF    MERCURIC 


CHLORIDE    IN 
ACETONE. 


ETHYL   ACETATE    AND    IN 


(Etard;  von  Laszcynski  —  Ber.  27,  2285,  '94;  Krug  and  McElroy  —  J.  Anal.  Ch.  6,  186,  '92;  Linebar- 
ger  —  Am.  Ch.  J.  16,  214,  94;  Aten  —  Z.  physik.  Ch.  54,  121,  '05.) 

NOTE.  —  The  results  obtained  by  the  above  named  investigators 
were  calculated  to  a  common  basis  and  plotted  on  cross-section  paper. 
The  variations  which  were  noted  could  not  be  satisfactorily  harmonized, 
and  therefore  all  the  results  are  included  in  the  following  table. 


SOLUBILITY. 


In  Ethyl  Acetate. 


In  Acetone. 


Grams  HgCl2  per  TOO  Grams  Solution. 


Gms. 


per  TOO  Gms.  Solution. 


tl    .  t  

Laszcynski. 

Aten.    Linebarger. 

N           1  

Etard.     K  and  McE.  Laszcynski.         Aten. 

Etard. 

—  10 

. 

23- 

O 

40 

44-0* 

57 

.0 

O 

22 

•  O 

23- 

2 

32 

.0 

40 

49-7 

43-o* 

61 

•7 

+  10 

22 

.2 

23- 

5 

32 

•5 

40 

52.0 

51.0^-58.9! 

6! 

•7 

20 

22 

•5 

23- 

4 

32 

•7 

40 

54 

58-  st 

61 

•7 

25 

22 

•7 

23 

5 

33 

.0 

40 

37-4       55-2 

58.  2  f 

61 

-7 

30 

23 

.0 

. 

33 

.2 

40 

...          ... 

61 

•7 

40 

23 

•5 

. 

33 

•5 

40 

61 

-7 

50 

24 

.0 

33 

•5 

41 

61 

•7 

60 

24 

•7 

. 

. 

42-5 

...          ... 

61 

•7 

80 

26 

.0 

45-2 

61 

•7 

IOO 

.  « 

48.0 

1  20 

. 

. 

50.8 

... 

. 

150 

. 

. 

. 

55-o 

... 

(*) 

Solid 

phase  HgCl2(CH3)2CO. 

(t)  Solid 

Phase  HgCl2. 

loo  grams  absolute  acetone  dissolve  143  grams  HgCl2  at  18°. 

(Naumann  —  Ber.  37,  4332,  '04.) 


SOLUBILITY  OF  MERCURIC  CHLORIDE  IN  SEVERAL  SOLVENTS. 

(Arctowski  —  Z.  anorg.  Ch.  6,  267,  '94;  von  Laszcynski;  Sulc.  —  Z.  anorg.  Ch.  25,  401,  'oo.) 


In  Carbon  Bisul- 
phide (A.). 


... 

Gms.  HgCl2 
per  100  Gms. 
Solution. 

—  10 

O-OIO 

0 

O.OlS 

10 

O.O26 

15 

0.032 

20 

0.042 

25 

30 

0-053 
0.063 

In  Benzene 
(von  L.). 


In   Several   Solvents 
at  18-20°  (S.). 


Gms.  HgCl2 

Gms.  HgCl2 

t  °. 

per  100  Gms. 

Solvent. 

per  100  Gms. 

Solution. 

Solvent. 

IS 

o-537 

CHBr3 

0.486 

41 

0.616 

CHC13 

0.106 

55 

0.843 

CC14 

O.OO2 

84 

1.769 

C2H5Br 

2  .OIO 

C2H4Br2 

1-530 

I95  MERCURIC    CHLORIDE 

SOLUBILITY   OF   MERCURIC   CHLORIDE    IN   ABSOLUTE   ETHYL   ETHER. 

(Etard;  Laszcynski ;  Kohler  —  Z.  anal.  Ch.  18,  242,  '79.) 


to          Cms.  HgCl2  per            t<J         Cms.  HgCl2  per                 .0          Cms.  HgCI2  per 
100  Gms.  Solution.             '     100  Gms.  Solution.                        100  Cms.  Solution. 

—  20 

6.0 

60 

6.0 

90 

7-5 

O 

6.0 

70 

6.4 

100 

8.0 

2O 

6.0 

80 

7.0 

no 

8-5 

SOLUBILITY  OF  MERCURIC  CHLORIDE  AND  OF  DOUBLE  MERCURIC  AND 
TETRA  METHYL  AMINE   CHLORIDE    (CH3)4NC1.6HgCl2  IN  AQ.  ETHER 

AT    I  7    .        (Stromholm  —  J.  pr.  Ch.  [2]  66,  443,  '02;  Z.  physik.  Chem.  44,  64,  '03.) 
Molecular  Concentration  per  IJter.  Grams  per  Liter  of  Solution. 


H20. 

HgCl2  (*). 

HgCl2  (f). 

H20. 

HgCl2  (*). 

HgCl2  (f). 

O-O 

O.I5I5 

0.0342 

O 

41  .16 

9.26 

0.0656 

0-1795 

0-0428 

1.18 

48.64 

II  .60 

O.I3II 

o  .  2069 

0-0516 

2.36 

56.08 

I4.OO 

0-1956 

0.2339 

o  .  0603 

3-52 

63-38 

16.34 

0.26ll 

o  .  2489 

0.0690 

4.70 

70.16 

18.70 

0.3267 

0.2849 

0.0779 

5.88 

77-20 

21  .10 

0.3922 

0.3100 

0-0866 

7.06 

84.02 

23.48 

(*)  Results  in  this  column  are  for  solutions  in  contact  with  the  Solid  Phase  HgCl2.     (f)  Results  in 
this  column  are  for  solutions  in  contact  with  the  Solid  Phase  (CH3)4NC1.6HgCl2. 


SOLUBILITY  OF  MERCURIC  CHLORIDE  AND  OF  DOUBLE  MERCURIC  AND 
TETRA  METHYL  AMINE   CHLORIDE   IN  ALCOHOL-ETHER  SOLUTIONS 

AT    17°.  (Stromholm.) 

Grams  C2H5OH  per  Liter.    Grams  HgCl2  (*)  per  Liter.     Grams  HgCl2  (f)  per  Liter. 

o.o  41.16  9.26 

4.58  50.00  11.87 

9.16  58-76  I4-38 

13.74  66.96  16.90 


SOLUBILITY  OF  DOUBLE  MERCURIC  CHLORIDES  IN  AQUEOUS  AND  PURE 

ETHER  AT   16.6°. 

(Stromholm.) 
Mol.  Cone,  of  HgCl2  per  Liter  of:  Gms.  HgClo  per  Liter  of: 

Pure        Aq.           Aq.          Aq.  Pure      Aq.  Aq.         Aq.                   T§°ll(J 

Ether.     Ether  Ether  Ether  Ether.   Ether  Ether     Ether 

(i).          (2).           (3).  (4)-  (5).         (6). 

0.1515  0.2387  0.2647  °-3T96  41.04  64.69  71.71   86.58  HgCl2 

0.0673  0.0673  0.1293  0.1617  l8-23   l8-23  35-°5  43-79  (CHa.CH3C2H4)2SC1.6HgC]2 

0.0404  0.0720  0.0835  0.1034  10.95    19.51  22.61    28.01  (CH3.C2H5CH3C2H4)2SC1.6HgCl2 

0.0342       .  .  .  0.0706      .  .  .  9.26     ...  19.10     ...  (CH3)4NC1.6HgCI2 

0.0264      .  .  .  0.0568      .  .  .  7.14     .  ..  15.39     .  .  .  (C2H5)3SC1.6HgCl2 

0.0209  0-0400  0.0460  0.0594  5.66  10.83  12.48   16.10  (CH3.C2H5)2SC1.6HgCl2 

0.0063        ...  0.0144      ...  1.70     ...  3.90     ...  (CH3)2.H2NC1.2HgCl2 

(i)  containing  0.21055  mol.  H2O  per  liter.  (2)  0.2756  irol.  H2O  per  liter.  (3)  0.421  mol.  H2O  per  liter 
(4)  containing  3.79  gins.  H2O  per  liter.    (5)  4.97  gms.  H2O  per  liter.   (6)  7.59  gms.  H2O  per  liter. 


MERCURIC    CHLORIDE 


196 


DISTRIBUTION  OF  MERCURIC  CHLORIDE  BETWEEN  WATER  AND 
TOLUENE  AT  24°. 

(Brown  —  J.  Physic.  Ch.  2,  50,  '98.) 

Gms.  HgCl2  per  100  cc.  Gms.  HgC^  per  100  cc. 

'    H-jO  QjHgCHa  H^O  C6H6C'H3 

Layer.  Layer.  Layer.  Layer. 

0.442      0.0270      1.816        0.130 

0.732         0-0488         3-766  0.292 

0.780       0.0542       3-754        0.298 
1.192       0.0812       6.688*       0.528* 

*  This  solution  saturated. 

MERCUROUS    CHLORIDE    HgCl. 

One  liter  water  dissolves  0.002  gram  HgCl  at  18°,  by  conductivity 
method. 

(Kohlrausch  —  Z.  physik.  Ch.  50,  356,  '04- '05.) 


SOLUBILITY  OF  MERCUROUS  CHLORIDE  (CALOMEL)  IN  AQUEOUS  SOLU- 
TIONS OF  SODIUM  CHLORIDE,  BARIUM  CHLORIDE,  CALCIUM 
CHLORIDE  AND  OF  HYDROCHLORIC  ACID  AT  25°. 

(Richards  and  Archibald  —  Proc.  Am.  Acad.  37,  345,  'oi-'oa.) 

Solid  phase  in  each  case.    Calomel  +  about  o.i  gram  of  mercury. 


In  Aqueous  NaCl. 


In  Aqueous  BaCl2. 


Sp.  Gr.  of 

Grams 

per  Liter. 

Sp.  Gr.  of 

Grams  per 

Liter. 

Solutions. 

NaCl. 

HgCl2.  ' 

Solutions. 

BaCl2. 

HgCl2. 

.  .  . 

5-85 

0.0041 

1.  088 

104.15 

0-044 

I  .040 

58.50 

O.O4I 

I-I34 

156.22 

0.088 

1.078 

II9.OO 

O.I29 

I.I74 

208.30 

O.IO7 

1.093 

148.25 

0.194 

1.263 

312.45 

0.231 

I  .142 

222-3 

0.380 

I.I88 

292.5 

0.643 

In  Aqueous  CaCl2 


In  Aqueous  HC1. 


Sp.  Gr.  of 

Grams  per  Liter. 

Sp.  Gr.  of 

Grams  per 

Liter. 

Solutions. 

CaCl2.                HgCl2. 

Solutions. 

HC1. 

HgCl2. 

39.96               O-022 

31.69 

0-034 

55-5            0.033 

36.46 

0-048 

I  .064 

m.o            0.081 

I  .042 

95-43 

0.207 

I  .105 

138.75          0.118 

I  .069 

158-4 

o-399 

I.I5I 

195.36          0.231 

I  .091 

209.2 

0.548 

I  .205 

257-52          0.322 

I  .114 

267.3 

0-654 

1-243 

324.67          0.430 

I  .119 

278-7 

0.675 

1-315 

432.9            0.518 

I.I32 

3*7-3 

0.670 

'•358 

499-5            0.510 

I-I53 

364.6 

0-673 

100 


grams  bromoform,  CHBr3,  dissolve  0.055  gram  HgCl  at  i8°-2o°. 

(Sulc.  —  Z.  anorg.  Ch.  25,  401,  'oo.) 


i97 


MERCURIC    CYANIDE 


MERCURIC    CYANIDE    Hg(CN)2. 


SOLUBILITY  IN  SEVERAL  SOLVENTS. 


Solvent. 

Water 


—0-45 
15.2 

IOI.I 

Abs.  Ethyl  Alcohol  19.5 
Abs.  Methyl  Alcohol  19.5 
Glycerine  15.5 


Gms.  Hg(CN)2  per 
100  Gms.  Solvent. 

about  1 1 .  o 
8.0 

10.1 
44.2 
27.0 


Observer. 

(Guthrie  —  Phil.  Mag.  [5]  6,  40,  '78.) 

(Wittstein.) 

(Griffiths.) 
(de  Bruyn  —  Z.  physik .  Ch.  10,  784,  '92 .) 


SOLUBILITIES  OF  MERCURIC  CYANIDE  DOUBLE  SALTS  IN  WATER  AND 

IN  ALCOHOL. 


Double  Salt. 

Hg(CN)2.2KCN 

Hg(CN)2.2TlCN 

Hg(CN)2.2TlCN 

2Hg(CN)2.CaBr2.5H2O  cold 

2Hg(CN)2.CaBr2.5H20  boiling 

Hg(CN)2.KCl.H2O 

Hg(CN)2.KBr.2H2O 

Hg(CN)2.KBr.2H20 

Hg(CN)2.BaI2.4H20 

Hg(CN)2.BaI2.4H20 

Hg(CN),KI 

Hg(CN)2.NaI.2H2O 

Hg(CN)2.SrI2.6H20 


Gms.  per  100  Grams. 


I; 

Water. 

Alcohol. 

v-'userver. 

cold 

22.7 

. 

1° 

12.6 

.  .  . 

(Fromuller 

—  Ber.  II,  92, 

10° 

9-7 

" 

" 

cold 

100.  0 

50.0 

(Custer.) 

boiling 

400.0 

IOO.O 

18° 

14.81 

(Brett.) 

18° 

7-49 

" 

boiling 

IOO.O  + 

.  .  . 

" 

cold 

6.42 

4.42 

(Custer.) 

boiling 

250.0 

62.5 

(90% 

Ale.) 

" 

cold 

6.2 

1.04 

(34°  B 

Ale.) 

(Caillot.) 

18° 

22.2 

15-4 

(90% 

Ale.) 

(Custer.) 

18° 

14-3 

25.0 

(90% 

Ale.) 

" 

SOLUBILITY  OF  MERCURIC  CYANIDE  IN  ORGANIC  SOLVENTS 

AT    l8°-20°. 
(Suk  —  Z.  anorg.  Ch.  25,  401,  'oo.) 

Solvent. 

Bromoform 

Carbon  Tetra  Chloride 
Ethyl  Bromide 
Ethylene  Di  Bromide 


Formula. 

G.  Hg(CN)2  per 
100  Gms.  Solvent. 

CHBr3 

O.O05 

CC14 

O-OOI 

C2H5Br 

0.013 

C2H4Br2 

0.001 

MERCURY    FULMINATE    C2HgN2O2. 
One  liter  of  water  dissolves  1.738-1.784  grams  C2HgN2O2  at  12°. 

(Holleman  —  Rec.  trav.  chim.  15,  159,  '96.) 

MERCURIC    IODIDE    HgI2. 

SOLUBILITY  IN  WATER. 

t  °.  Grams  HgI2  per  Liter.  Observer. 

l8  0-0004    (Conductivity  method)  (Kohlrausch  —  Z.  physik.  Ch.  50,  356,  fo4-'os.) 

17.5  O  .040  (Bourgoin  —  Bull.  soc.  chim.  [2]  42,  '84.) 

22  0.054  (Rohland  —  Z.  anorg.  Ch.  18,  328,  '98.) 


MERCURIC    IODIDE 


198 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  ALCOHOLS. 


Alcohol. 

Formula. 

t°. 

Sp.  Gr.  of 
Solution. 

G.  HgI2  per 
100  Gms. 
Alcohol. 

Observer. 

Methyl 

CH3OH 

15-20 

0.799 

3-24 

(Rohland.) 

it 

tt 

19-5 

3-16 

(de  Bruyn.) 

t( 

tt 

66  (b.  pt.) 

6.512 

(Sulc.) 

Ethyl 

C2H5OH 

15-20 

O.8lO 

1.42 

(Rohland.) 

a 

tt 

18 

1.48 

(Bourgoin.) 

ii 

tt 

19-5 

2.09 

(de  Bruyn.) 

tt 

25 

0.803 

2.19 

(HerzandKnoch.) 

tt 

it 

78  (b.  pt.) 

4.325 

(Sulc.) 

Propyl 

C3H7OH 

15-20 

0.816 

0.826 

(Rohland.) 

Amyl 

C5HUOH 

13 

0.66 

(Laszcynski.) 

« 

« 

7i 

3.66 

" 

tt 

tt 

100 

5.30 

« 

a 

tt 

133-5 

9-57 

« 

Iso  Propyl 

(CH3)2CH.OH 

81  (b.  pt.) 

.  .  . 

2.266 

(Sulc.) 

Iso  Butyl 

(CH3)2CHCH2OH 

105-107  (b.  pt 

,)    ... 

2-433 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  AQUEOUS  ETHYL  ALCOHOL: 
At  1 8°.  At  25°. 

(Bourgoin.)  (Herz  and  Knoch  —  Z.  anorg.  Ch.  45,  266,  '05.) 


Solvent 

Gms.  HgI2 

Wt.%  Alcohol 

HgI2  per  loo  cc.  Solution. 

Sp  Gr.  of 

per  Liter. 

in  Solvent. 

Millimols. 

Grams.  "     Solutions  25°/4( 

Abs.  Alcohol 

11.86 

IOO 

3.86 

J-754 

0.8033 

H2O  +  8o%9o°Alc. 

2.857 

95-82 

2  .56 

i  .162 

0.8095 

H2O+io.%9o°Alc. 

0.086 

92.44 

I  .92 

0.873 

0.8154 

86.74 

L38 

0.623 

o  .  8300 

78-75 

o-935 

0.425 

0.8405 

67.63 

0.45 

0.204 

0.8721 

SOLUBILITY  OF  MERCURIC  IODIDE  IN  ACETONE  IN  ETHYL  ACETATE 
AND  IN  BENZENE. 

(Sulc;  Krug  and  McElroy  —  J.  Anal.  Ch.  6,  186,  '92;  Laszcynski  —  Ber.  27,  2285,  '94.) 


In  Acetone. 


In  Ethyl  Acetate. 


In  Benzene. 


Gms.  HgI2 

Gms.  Hglo 

Gms.  HgI2 

t°.       per  loo  Gms. 
(CH3)2CO. 

t°.           per  TOO  Gms. 
CH3COOC2H6. 

t°.          per  loo  Gms. 
C6H« 

I               2.83 

—  2O 

1-49 

15               0-22 

18          3-36 

+  17-5 

I.56 

60          0.88 

25              2  .09  (K.andMcE.) 

21 

I  .64 

65          0.95 

40             4-73 

40 

2-53 

84          1.24 

58             6.07 

55 

3-i9 

80  (b.pt.)  0.825  (Sulc.) 

56  (b.pt.)  3  .  249  (Sulc.) 

76 

4-31 

74-78  (b.pt.)  4  .  20  (Sulc.) 


MERCURIC    IODIDE 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  CARBON  BISULPHIDE. 

(Linebarger  —  Am.  Ch.  J.  16,  214,  '94;  Arctowski  —  Z.  anorg.  Ch.  6,  267,  '94;  u,  274,  '95.) 


-ii6 

-  93 

-  86.5 
—   10 


Cms.  HgI2  per 
100  Gms.  Solution. 

0.017 
0.023 
O.024 
O.IO7 


-   5 
o 

+  5 
10 


Gms.  Hgl2  per 
100  Gms.  Solution. 

O.I4I 
0.173 
0.2O7 
0.239 


15 
20 

25 
30 


Gms.  HgI2  per 
100  Gms.  Solution. 

0.271 
0.320 
0.382 

0-445 


SOLUBILITY  OF  MERCURIC   IODIDE   IN   SEVERAL  ORGANIC  SOLVENTS. 

(Sulc  —  Z.  anorg.  Ch.  25,  401,  *oo.) 


Solvent. 

Chloroform 

Chloroform 

Bromoform 

Tetra  Chlor  Methane 

Tetra  Chlor  Methane 

Ethyl  Bromide 

Ethyl  Bromide 

Ethylene  Di  Bromide 

Ethyl  Iodide 

Ethylene  Di  Chloride 

Iso  Butyl  Chloride 

Methyl  Formate 

Ethyl  Formate 

Methyl  Acetate 

Acetal 

Epi  Chlor  Hydrine 

Hexane 


Formula. 

CHC13 

CHC13 

CHBr3 

CC14 

CC14 

C2H5Br 

C2H5Br 

C2H4Br2 

C2H5I    ' 

C9H4C12 

(CH3),.CHCH2C1 

HCOOCH3 

HCOOC2H5 

CH3COOCH3 

CH3CH(OC2H5)2 

CH2.O.CH.CHuCl 


t°. 

Gms.Hgl2per  ioo 

Gms.  Solvent. 

18-20 

O.O4O 

61  (b.  pt.) 

0.163 

18-20 

0.486 

18-20 

O.OO6 

75  (b.  pt.) 

0-094 

18-20 

0.643 

38°  (b.  pt.) 

o-773 

18-20 

0.748 

18-20 

2  .041 

85.5°  (b.  pt 

,)             1.200 

69 

0.328 

36-38     " 

1.166 

52-55     " 

2  ^50 

56-59     " 

2  .500 

105 

2  -OOO 

117 

6.II3 

67 

O.O72 

SOLUBILITY    OF   MERCURIC 


IODIDE    IN 
IODIDE. 


In  Ether. 

(Sulc;  Laszcynski.) 

4.0  Gms.  HgI2  per  ioo 

Gms.  (C2H6)20. 

o  0.62 

36  0.97 

35  (b.  pt.)  0.47  (Sulc) 


ETHER   AND    IN    METHYLENE 
In  Methylene  Iodide. 

(Retgers  —  Z.  anorg.  Ch.  3,  253,  '93.) 


15 

IOO 

180 


Gms.  HgI2  per  ioo 
Gms.  CH2I2. 

2-5 

16.6 

58.0 


SOLUBILITY  OF  MERCURIC  IODIDE  IN  FATTY  BODIES. 

(Mehu  —  J.  pharm.  chim.  [5]  12,  249,  '85.) 
Solvent. 

Bitter  Almond  Oil 

Bitter  Almond  Oil 

Castor  Oil 

Castor  Oil 

Nut  Oil 

ioo  grams  oil  of  bitter  almonds  dissolve  5.0  grams  HgI2.KI  at  25°. 

(Mehu.) 


.0      Gms.  HgI2  per 
'  ioo  Gms.  Solvent, 

Solvent. 

to         Gms.  HgI2  per 
'     ioo  Gms.  Solvent. 

25 

o-5 

Vaseline 

25 

0.025 

IOO 

Vaseline 

IOO 

O-2O 

25 

4-0 

Poppy  Oil 

25 

I  -O 

IOO 

20-0 

Olive  Oil 

25 

0-4 

IOO 

I  .2 

Carbolic  Acid 

IOO 

2.0 

MERCURY    OXIDE 


200 


MERCURY    OXIDE    HgO. 

SOLUBILITY  IN  WATER. 

(Schick  — Z.  physik,  Ch.  42,  163,  'oi-'o2.) 
Grams  per  1000  cc.  Solution. 


te. 

25 
IOO 


0.0518  yellow  HgO  0.05 13  red  HgO 

0.410   yellow  HgO  0.379  red  HgO 

EQUILIBRIUM  IN  THE  SYSTEM,  MERCURY  OXIDE,  SULPHUR  TRI- 
OXIDE,  WATER. 

(Hoitsema  —  Z.  physik.  Chem.  17,  651,  '95.) 

Results  expressed  in  molecules  per  sum  of   100  molecules  of  the 
three  components  of  the  system. 


Results  at  25°. 


Results  at  50* 


Liqu 

d  Phase. 

Solid 

Liquid  Phase. 

Solid 

'     H20. 

SO3. 

HgO. 

Phase. 

'   H20. 

SO3. 

HgO. 

Phase. 

98 

•5 

I 

.24 

o-33 

3HgO.SO3 

98 

•9 

0.96 

o. 

17 

3HgO.SO3 

96 

.6 

2 

•49 

0.92 

" 

96 

.0 

3-05 

0.93 

94 

•4 

3 

•93 

1.65 

" 

93 

.2 

4.92 

I  . 

90 

" 

93 
94 

•9 

•4 

4 
4 

.24 

•52 

1.85 

2.12 

3HgO.SO3  and 
3Hg0.2SO3.2H2O 

92 
92 

.8 
.8 

5.10 
5.16 

2  . 
2  . 

09 
06 

.. 

93 

•4 

4 

•65 

1.94 

3HgO.2SO3.2H20 

92 

•5 

5-34 

2  . 

12 

" 

92 

.9* 

4 

.81 

2  .29 

3HgO.S03 

92 

.2 

5-57 

2  . 

2O 

3HgO.SO3  and 

92 

•9 

5 

.11 

1.98 

3HgO.2SO3.2H2O 

3Hg0.2SO3.2H2O 

92.3* 

5 

.20 

2-54 

3HgO.SO3 

92 

.1 

5-75 

2  . 

II 

3HgO.2SO3.2H2O 

92 

•3 

5 

•58 

2.09 

3HgO.2SO3.2H2O 

92 

.0 

5.80 

2. 

16 

" 

92 

.1 

5 

.81 

2.08 

x           " 

91 

.2* 

6.27 

2  . 

56 

3HgO.SO3and 

91 

•9 

5 

•97 

2.90 

3HgO.S03 

HgO.S03 

91 

•9 

6 

.15 

2  -05 

3HgO.2S03.2H2O 

91 

•5 

6-34 

2  . 

19 

3HgO.2SO3.2H2O 

91 

•3 

6 

•54 

2.13 

" 

and  HgO.S03 

91 

.2 

6 

•77 

2  .02 

HgO.S03.H2O 

91 

•3* 

6-37 

2  . 

30 

HgO.SO3 

91 

•3 

6 

.90 

1.  80 

u 

91 

.6 

6.69 

I  . 

75 

" 

91 

•3 

7 

.67 

I  .01 

« 

91 

.1 

8.32 

o. 

57 

" 

•3 

7 

.84 

0.89 

HgO.S03.H20 

89 

.6 

10.2 

o. 

23 

« 

91 

.0 

8 

•36 

0.69 

and  HgO.SO3 

31 

.6 

68.4 

o. 

03 

u 

90 

•5 

8 

•95 

o-53 

HgO.SO3 

89 

.2 

10 

.6 

O.22 

" 

75 

.8 

24 

.2 

trace 

" 

39 

.2 

60 

•7 

trace 

" 

*  Indicates  unstable  equilibrium. 

MERCUROUS    SULPHATE    Hg2SO4. 

SOLUBILITY  IN  WATER,  IN  SULPHURIC  ACID  AND  IN  POTASSIUM 
SULPHATE  AT  25°. 

(Drucker  —  Z.  anorg.  Ch.  28,  362,  '01;  Wright  and  Thomson  —  Phil.  Mag.  [5]  17,  288;  19,  i,  '84-'8s; 
Wilsmore  —  Z.  physik.  Ch.  35,  505,  'oo.) 

Hg2SO4.per  Liter. 


Solvent. 


Water 

Aq.H2SO4  (  i  .96  gms.  per  liter) 
Aq.H2SO4 .(  4.90  gms.  per  liter) 
Aq.H2SO4  (9.80  gms.  per  liter) 
Aq.K2SO4  (34.87  gms.  per  liter) 


Gram  Mols. 

11.71   10 

8.3I        ' 

8.78        ' 

8.04     " 
9-05     * 


Grams. 

O  .058(0.047  W.andT.,  0x239  W.) 

0.041 

0.044 

O.O4O 

0.045 


201 


METHANE 


METHANE     CH4. 


SOLUBILITY  IN  WATER. 

(Winkler  —  Ber.  34,  1418,  '01.) 


o  0.05563  0.05530  0.00396 
5  0.04805  0.04764  0.00341 
10  0.04177  0.04127  0.00296 
15  0.03690  0.03628  0.00260 

20   0.03308   0.03233   0.00232 
25   O.O3OO6   0-02913   O.OO2O9 
30   0-02762   0-02648   O.OOI9I 

40   0.02369   0.02198   O.OOI59 
50   O.O2I34   0.01876   0.00136 
60   0.01954   O.OI57I   O.OOII5 
7O   0.01825   O.OI265   O.OOO93 
80   O.OI77O   0.00944   O.OOO70 
9O   O.OI735   0.00535   O.OOO40 

100  0.01700  o.ooooo  o.ooooo 

For  the  values  of  /3,  /3'  and  q  see  Ethane,  page  133. 


SOLUBILITY  OF  METHANE  IN  METHYL  ALCOHOL  AND  IN  ACETONE. 

(Levi  —  Gazz.  chim.ital.  II,  513,  '01;  abs.  in  Z.  physik.  Ch.  41,  no,  '02.) 

In  methyl  alcohol  /  (Ostwald  expression,  seepage  105)   =  0.5644  — 
0.0046  t  —  o.  00004  t2. 

In  acetone  /  (Ostwald  expression)  =  0.5906  —  0.00613^  —  0.0000146^. 
From  which  is  calculated  the  following  values: 


In  Methyl  Alcohol. 


In  Acetone. 


o  0.5644 
10  0.5144 
20  0.4564 

30  0.3904 

40  0.3164 
50  0.2344 

60  0.1444 
70  0.0464 

o  o  .  5906 
10  0.5278 
20  0.4622 

30  0.3936 

40  0.3220 
50  0.2476 
60  o.i  702 
70  0.0900 

Tetra   Chlor    METHANE    CC14    (Carbon  Tetra  Chloride) . 
SOLUBILITY  IN  WATER. 

(Rex  — Z.  physik.  Chem.  55,  355,  '06.) 
t  °.  o°.  10°.  20°. 

Grams  CC14  per  100  gms.  H2O         i  .097        0.083        0.080 


30°. 
0.085 


Tri    Phenyl    METHANE    CH(C6H6)3. 


SOLUBILITY 

(Hartley  and  Thomas  —  J 

By  synthetic  method,  see  page  9. 


Gms. 

CH(C6H5)3  Mol.  per 
t°.       per  100          cent 

Gms.  So-  CH(C6H5)3. 
lution. 


23.0 

35-3 
43-o 
52.1 
61  .4 
66.0 
68.7 
70.1 

5-4 

9-5 
!3-5 
21.9 

36-5 
47.2 

54-8 
64.6 

1.85 
3-8 
5-6 

9-7 
17.8 

25-4 
31.6 
40.9 

«...  . 
p?olld 
Phase' 


s  ... 
£r  c 


IN  ANILIN. 

Ch.  Soc.  89,  1026,  '06.) 


Gms. 

CH(C6H5)3  Mol.  per 
t  °.         per  100          cent 

Gms.  So-  CH(C6H6)3. 

lution. 

71.3      67-9  44-6     CH^>3.CeH5oNH2 

71.6     71.7  49-1 

71.2  76.3  55.1 
70.6     78.3  57.9 

71.6      82.1  63. 5  CH(C«jH5)3  monoclinic 

74.3  84.9  68.2 

82.1       91.7  80.9 

87.3      96.1  90.2 


Tri   Phenyl    METHANE 


202 


SOLUBILITY  OF  TRI  PHENYL  METHANE  IN  BENZENE. 

(Linebarger  —  Am.  Ch.  J.  15,  45,  '93.)                                 (Hartley  and  Thomas.) 
Gms.                                                                              Gms.                •»,  , 

f.      C" 

,Jtnu«ti5>3  PC 
'^QHe"13 

Solid  Phase.                   t°.          ViooGt£ 
Solution. 

per  cent       Solid  Phase. 
'  CH(C6H6)3. 

3-9 

3  90 

C6H6+CH(C6H5)3.C6H8      33 

12  .6 

4-4 

CH(C6H6)3.C6H8 
rhombs 

4-0 

4.06 

CH(C6H6)3-C6H6                    49  .  4 

24.0 

8.8 

12-5 

5-i8 

65.6 

38-9 

17  .2 

" 

16.1 

6.83 

73-8 

57-5 

30.2 

" 

19.4 

7.24 

77.1 

67.4 

39-7 

" 

23.1 

8-95 

77-9 

76-3 

5°  -7 

" 

37-5 
42  .0 

10.48 
19.61 

(C6H5)3CH.C6H8                    7?    ,- 
+  CH(C6HS)3                     1  7'5 
CH(C6H6)3                             70-2 

80.2 
84.1 

56-4 
62.8 

:: 

44.6 

22  .64 

74-6 

87-5 

69.1 

CH(C6H5)3. 
monoclinic 

50.1 

30.64 

76.0 

89.0 

72.2 

" 

55-5 

40.51 

78.8 

9o-5 

75-3 

" 

71  .0 

I4O.OO 

82.3 

93-i 

81.3 

11 

76.2 

319.67 

86.6 

95-7 

87.8 

" 

NOTE. — Hartley  and  Thomas  call  attention  to  the  inaccuracy  of  Linebarger 's  results  and  the  cor- 
rectness of  Kuriloff 's  determinations  (Z.  physik.  Chem.  22,  547,  '97). 


SOLUBILITY  OF  TRI  PHENYL  METHANE  IN  CARBON  BISULPHIDE. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  570,  '94;  below  —  80°,  Arctowski  —  Z.  anorg.  Ch.  n,  273,  '95.) 


Gms.  CH(C6H5 

t  °. 

per  100  Gms. 

Solution. 

—  113 

-5        0.98 

—  102 

1.24 

-    91 

1.56 

-    83 

1.91 

-    60 

3-4 

Gms.  CH(C6H5)3 
t°.             per  100  Gms. 
Solution. 

-40 

7-5 

—  2O 

13  .  7 

O 
+  10 

25.8 
38.7 

2O 

43-2 

30 

52-9 

40 
5° 

60 
70 
80 


Gms.  CH(C6H6)3 

per  100  Gms. 

Solution. 


63 
72 


78.6 
85.6 
92  .  2 


SOLUBILITY  OF  TRI  PHENYL  METHANE  IN  HEXANE  AND  IN 


CHLOROFORM. 

(Etard.) 


Gms.  CH(C6H5)3  per  100  Gms. 
Solution  in: 


Hexane  . 

Chloroform. 

-5o 

10-5 

-30 

I  .2 

15.2 

—  20 

1.6 

I9.O 

—  10 

2  .2 

23-5 

0 

3-5 

28.9 

+  10 

5-6 

35-o 

20 

8-3 

4i-5 

Gms.  CH(C6H5)3  per  100  Gms. 
Solution  in: 


Hexane. 

Chloroform. 

30 

12-5 

48.8 

40 

2O-  0 

56.1 

50 

25.8 

63.8 

60 

45-7 

71.7 

70 

62  .0 

79-8 

80 

78-5 

87.2 

90 

97.0 

203 


Tri   Phenyl    METHANE 


SOLUBILITY  OF  TRI  PHENYL  METHANE  IN  PYRIDINE. 

(Hartley  and  Thomas  — J.  Ch.  Soc.  89,  1028,  '06.) 

Synthetic  method  used,  see  note,  page  9. 


Cms.  Mol. 

CH(QjH5)3        per  Solid 

penooGms.     cent  Phase. 

Solution.    CH(C6H5)3. 


22.8 
31'? 

37-9 
48.7 


46.2 

53-3 
57-6 
66.6 
70.1 


22.0 
27.2 
30-7 

39-5 
43-5 


CH(C6H6)3 

„       monoclinic 


Gms.  Mol. 

CH(C«H6)3      per  Solid 

penooGms.     cent.  Phase. 

Solution.    CH(C6H6)3. 


59-3 

67.8 
72.8 
80.6 

86.8 


75-6 
81.9 

85-7 
9*-S 
95-8 


CH(Q»H5)3 


59  7 
66.4 

77-2 
88.1 


SOLUBILITY  OF  TRI  PHENYL  METHANE 

(Hartley  and  Thomas.) 


IN: 


Gms. 

Pyrrole. 

Mol. 

Gms. 

Thiophene. 

Mol. 

to      CH(C6H6)3       per                     Solid 
'  per  i  oo  Gms.     cent                   Phase. 
Sol.         CH(C6H5)3. 

to      CH(C6H5)3       per                   Solid 
'   per  ioo  Gms.    cent                   Phase. 
•    Solution.   CH(C6H5)3. 

24 

.6 

24 

•3 

8 

.  I       CH(C6H5)3.C4H4NH 
rhombs 

25 

•7 

26.O 

10 

.8         CH(C6H5)3 

i 

29 

.0 

29 

.8 

10 

•4 

33 

•5 

31-1 

*3 

•5 

31 

•5 

33 

•4 

12 

.1 

44 

.0 

43-6 

21 

.1 

36.8 
42.7 

40 
49 

.6 
.1 

2O 

.8      CH(C6H6)3 
„    monoclinic 

47 
53 

.6 

•5 

48.4 
58.7 

24 
32 

4 
•9 

46 

•9 

56 

.0 

25 

•9 

57 

•4 

70.2 

44 

•7 

53 

.2 

63 

•9 

32 

.8 

57 

.6 

74-8 

50 

.6 

60 

•  O 

72 

•3 

41 

.8 

62 

•7 

78.7 

56 

.0        CH(C6H5)3 

63 

•9 

76 

•7 

47 

•4 

67 

.0 

81.9 

60.8 

68 

•5 

81 

•9 

55 

.6 

67 

.2 

82.1 

61 

•3 

71 

.1 

84 

•4 

59 

74 

.2 

87.4 

70 

•5 

80 

.0 

91 

•5 

74-8 

79.0 

90-3 

76 

•3 

89 

.2 

97 

.6 

91 

.8 

87 

.2 

96.2 

89 

•9 

rhoml 


METHYL    ACETATE,    Butyrate    and    Propionate. 
SOLUBILITY  IN  WATER  AT  22°. 

(Traube  —  Ber.  17,  2304,  '84.) 

ioo  grams  H2O  dissolve   25.0  grams  CH3COOCH3;  1.7  grams  C3H7 
COOCH3;  5.0  grams  C2H5COOCH3. 


METHYL    IODIDE,  Methylene  Chloride  and  Methylene  Bromide. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Rex  —  Z.  physik.  Chem.  55,  355,  '06.) 

Grams  per  ioo  Grams  H2O. 


O 
10 
20 
30 


CH3I. 

CH2C12. 

CH2Br2. 

i-565 

2-363 

I-I73 

1.446 

2  .122 

I  .146 

1.419 

2  .OOO 

I.I48 

1.429 

1.969 

I.I76 

METHYL  BUTYRATE,       204 

METHYL  BUTYRATE,  METHYL  VALERATE. 

SOLUBILITY  OF  EACH  IN  AQUEOUS  ALCOHOL  MIXTURES. 

(Bancroft  —  Phys.  Rev.  3,  193,  '95.) 

ioo  cc.  H2O  dissolve  1.15  cc.  methyl  butyrate  at  20°. 

cc.  Alcohol  cc-  H2°  Added  *  cc.  Alcohol        cc.  H2O  Added  * 

in  Mixture.      Butyrate.  Valerate.  "*  Mixture.  Valerate. 

3  2.34  1-66  27  41.15 

6  -         6.96  5.06  30  52.37 

9  12.62  9.03  33  62.25 

12  19-45  J3-4o  36  74.15 

15  28.13  18.41  39  91.45 

18  33-8o  24.00  42                 oo 

21  55-64  3°-°9 

24  oo  36,72 

*  cc.  H2O  added  to  cause  the  separation  of  a  second  phase  in  mixtures  of  the  given  amounts  of  ethyl 
alcohol  and  3  cc.  portions  of  methyl  butyrate  and  of  methyl  valerate  respectively. 

METHYL    ETHYL    KETONE    CH3.CO.C2HS. 
SOLUBILITY  IN  WATER. 

(Rothmund  —  Z.  physik.  Chem.  26,  475,  '08.) 

By  synthetic  method,  see  Note,  page  9. 

0  Gms.  Ketone  per  ioo  Cms.  0  Cms.  Ketone  per  ioo  Gms. 

Aq.  Layer.        Ketone  Layer.  Aq.  Layer.        Ketone  Layer, 

—  io  34.5  89.7  90  16.1  84.8 

-f-io  26.1  90.0  no  17.7  80.0 

30  21.9  89.9  130  21.8  71.9 

50  17.5  89.0  140  26.0  64-0 

70  16.2  85.7  151.8  (crit.  temp.)44-2 

MOLYBDENUM    TRIOXIDE    MoO3. 

ioo  gms.  cold  H2O  dissolve  0.187  gm-  MoO3. 

(Dumas;  Buchlolz.) 

ioo  gms.  hot  H2O  dissolve  0.104  gm.  MoO3. 

(Hatchett.) 

MORPHINE   C17H19NO3.H2O. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.;  Mviller  —  Apoth.-Ztg.  18,  257,  '03.) 

Gms.  Morphine  per  ioo  Gms. 

Solvent.    Gms.  Morphine  per  ioo  Gms.  Solution.        Solvent.  Solution. 

At  i8°-22°.  At  25°.          At  8o6.  'At  i8°-22°. At  25°. 

Water  0.0283     0.030       0.0961  Chloroform        0.0655  °-°555 

Alcohol  ...        0.600       1.31(60°)     Amyl  Alcohol        ...  0.8810 

Ether  0.0131     0.0224  ...  Ethyl  Acetate   0.1861  0.1905 

Ether  sat.  with  Petroleum 

H2O  0.0094        ...  ...  Ether  0.0854 

H2O  sat.  with  Carbon  Tetra 

Ether  0.0447        •••  •••  Chloride         0.0156  0.032(17°) 

Benzene  0.0625        •  •  •  •  •  •  Glycerine  0.45  (15.5°) 


205  MORPHINE 

SOLUBILITY   OP   MORPHINE   IN   AQUEOUS   SOLUTIONS   OF   SALTS   AND 
BASES  AT  ROOM  TEMPERATURE,  SHAKEN  EIGHT  DAYS. 

(Dieterich  —  Pharm.  Centrh.  31,  395,  '90.) 

In  N/io  Salt  or  Base.  In  N/i  Salt  or  Base. 

Grams  per  Liter.  Grams  per  Liter. 


|.  csau  or  case.           <• 

Salt  or  Base. 

Morphine. 

Salt  or  Base. 

Morphine. 

NH4OH 

3-SI 

O.2O 

35-08 

0-505 

(NH4)2C03 

4.80 

0.031 

48.03 

O.O4O 

KOH 

4.62 

2.78 

46.16 

.  .  . 

K2C03 

6.92 

O-2O 

69.15 

o-379 

KHCO3 

IO.O2 

O.O24 

100.16 

0.040 

NaOH 

4-00 

3-33 

40.05 

.  .  . 

Na2CO3 

5-30 

0.09 

53-03 

0.14 

NaHCO3 

8.41 

0.032 

84.06 

0.044 

Ca(OH)2  (sat.) 

I  .00  (25°) 

MORPHINE  ACETATE  CH3COOH.C17H19NO3.3H2O,  Morphine 
Hydrochloride  HC1.C17H19NO3.3H2O,  Morphine  Sulphate  H2SO4. 
(C17H19NO3)2.5H2O,  and  Apo  Morphine  Hydrochloride  HC1.C17 
H17N02. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.) 
Grams  per  100  Grams  of  Solvent. 


Solvent. 

Acetate. 

Hydrochloride. 

Sulphate. 

Apo  M.  Hydrochloride. 

'25° 

80°. 

25°. 

80°, 

25°. 

80° 

25°- 

80°.' 

Water 

44- 

9 

50.0 

5-8l 

200. 

0 

6-53 

166. 

6 

2-53 

6.25 

Alcohol 

4- 

6 

40.0* 

2.4 

2. 

8* 

0.22 

0. 

53* 

2.62 

3-33 

Chloroform 

o. 

21 

.       .      0 

.  .  . 

.  . 

. 

. 

. 

0.026 

Ether 

.  .  , 

.  .  . 

.  .  . 

.  . 

. 

.  .  . 

.  . 

°-°53 

Glycerine 

19. 

2 

20.  Of 

.  .  • 

*  60°.  1 15.5°. 

ioo  gms.  H2O  dissolve    1.69   gms.  apo  morphine  hydrochloride  at 
15.5°,  and  2.04  gms.  at  25°. 

ioo  gms.   90%    alcohol  dissolve   1.96   gms.  apo   morphine    hydro 

Chlorde  at  2  5°.  (Dolt  —  Pharm.  J.  [4]  22,  345,  '75-) 

ioo  gms.  H2O  dissolve  4.17  gms.  morphine  sulphate  at  15°. 

(Power  — Am.  J.  Pharm.  March,  '82.) 

MUSTARD  OIL    Allyl  Isosulphocyanic  Ester  CS:NC3H5 

SOLUBILITY  IN  SULPHUR  BY  SYNTHETIC  METHOD.    See  Note,  p.  9. 

(Alexejew— Ann.  Physik.  Chem.  28,  305,  '86.) 

Grams  Mustard  Oil  per  ioo  grams. 


Sulphur  Layer.  Mustard  Oil  Layer. 

90  10  72 

IOO  12  67 

no  15  62 

120  23  51 

124  (crit.  temp.)  35 


a NAPHTHYLAMINE 


206 


a  NAPHTHYLAMINE  p  Sulphonic  Acid  (Naphtion  Acid),  i  :  4 
«  C10H6NH2.SO2H  and  a  Naphthalamine  o  Sulphonic  Acid,  i  :  2 
a  C10H6NH2.S02H. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Dolinski  —  Ber.  38,  1836,  '05.) 


O 
10 
20 

30 
40 


Gms.  per  100 

Gms.  H2O. 

Gms.  per  loojGms.  H2O. 

p  Sulphonic 

o  Sulphonic 

t  °. 

p  Sulphonic 

o  Sulphonic 

Ac. 

Ac. 

Ac. 

Ac. 

0.027 

O.24 

50 

0.059 

0.81 

0.029 

0.32 

60 

0.075 

I  .OI 

0.031 

0.41 

70 

0.097 

I  .37 

0.037 

0.52 

80 

0.130 

I.  80 

0-048 

0.65 

90 

0.175 

2  .40 

IOO 

o  .228 

3  -19 

NAPHTHALENE    C10H8. 

SOLUBILITY  IN  METHYL,  ETHYL,  AND  PROPYL  ALCOHOLS.  . 

(Speyers — Am.  J.  Sci.  [4]  14,  294,  '02  ;  at  19.5°,  de  Bruyn  —  Z.  physik.  Chem.  10,  784,  '92  ;  at  n°,  Timo 
feiew  —  Compt.  rend.  112,  1137,  '91.) 

The  original  results  were  calculated  to  a  common  basis,  plotted  on 
cross-section  paper,  and  the  following  table  read  from  the  curves. 


In  Methyl  Alcohol. 

0 

Wt.  of  i  ci 

Gms.  C10H8 

Solution. 

CH^OH"' 

O 

0.8194 

3-48 

10 

0.812 

5-6 

2O 

0.807 

8.2 

25 

0.805 

9.6 

30 

0.804 

II  .2 

40 

0.805 

16.2 

50 

0.813 

26.O 

60 

0.837 

5O.O 

65 

0.870 

70 

0.9023 

(68°)     .'.'.' 

In  Ethyl  Alcohol. 


In  P-opyl  Alcohol. 


Wt.  of  i  cc. 
Solution. 

Gms.  C10H8 
per  zoo  Gms 
C2H6OH. 

0.8175 

5-o 

0.814 

7-o 

O.SlO 

9.8 

0.809 

"•3 

0-809 

13-4 

0.812 

19.5 

0.822 

35-o 

0.855 

67.0 

0.890 

96.0 

0.930 

179.0 

Wt.  of  i  cc. 
Solution. 

0.8285 

0.824 

0.821 

0.82O 

O.82O 

0.823 

0-837 

0.867 

0.897 

0-933 


Gms.  Cjo-hs 

per  100  Gms. 

C3H7OH. 

4-45 
5-6 

8.2 

9.6 

xx  .4 

16.4 
26.0 
50.0 

80.0 

'34-1  (68.5°) 


SOLUBILITY  OF  NAPHTHALENE  IN  AQUEOUS  ACETONE. 

(Cady  — J.  Physic.  Ch.  2,  168,  '98.) 


Grams  per  100  Grams  Solution. 


1  
Acetone. 

Water. 

Naphthalene. 

IO.O 

89.92 

0.05 

19.91 

80.0 

O.O9 

29.92 

69.67 

O.4I 

40.8l 

58.22 

0-97 

48.67 

48.68 

2  -65 

57-43 

36.64 

5-93 

60.43 

25-75 

13.82 

65-5 

55-3 

45 

38 

32.2 

28.5 

28.2 


The  isotherms  for  intervals  of  10°  lie  so  close  together  that  they 
are  practically  indistinguishable  for  the  greater  part  of  their  length. 


207 


NAPHTHALENE 


SOLUBILITY  OF  NAPHTHALENE  IN: 


Chloroform. 

Carbon  Tetra 
Chloride. 

Carbon      Di 
Sulphide. 

(Speyers;  Etard.) 

(Schroder  —  Z.  physik.  (Arctowski  —  Compt. 
Ch.  n,  457,  '93.)     rend,  121,  123,  '95;  Etard.) 

Wt.  of  i  cc. 
Solution. 

Gms.  CioHg  per 
100  Grams 
CHC13. 

Gms.  CioHg  per 
100  Gms.  Sat. 
Solution  . 

Gms.  CioHg  per 
100  Gms.  Sat. 
Solution  . 

.  .  . 

O.62 

I.38 

2-3 

.  .  . 

8.8 

.  .  . 

6.6 

15.6 

14.1 

1-393 

19-5 

9-0 

19.9 

1-355 

25-5 

14-0 

27-5 

1.300 

31.8 

20.  o 

36-3 

1.280 

35-5 

23.0 

41  .0 

1-255 

40.1 

26.5 

46.0 

i  .205 

49-5 

35-5 

57-2 

i  .150 

60.3 

47-5 

67.6 

i  .090 

73-i 

62.5 

79-2 

i  .040 

87.2 

80.0 

9o-3 

-108 

-  82 

-  5° 

-  30 
—   10 

o 

+    10 
20 

25 

3° 
40 

5° 
60 
70 

NOTE.  —  Speyers'  results  upon  the  solubility  of  C10H8  in  CHQ3, 
when  calculated  to  grams  per  100  grams  of  solvent,  agree  quite  well 
with  Etard's  (Ann.  chim.  phys.  [7]  2  570,  '94  figures,  reported  on  the 
basis  of  grams  C10H8  per  100  grams  saturated  solution. 


Benzene. 


SOLUBILITY  OF  NAPHTHALENE  IN: 

(Schroder;  Etard;  Speyers.) 

Chlor  Benzene.  Hexane.  Toluene. 


t°. 

Gms.  CioHg 
per  zoo  Gms. 
Solution. 

Gms.  CioHs 
per  100  Gms. 
Solution. 

Gms.  CioHg 
per  100  Gms. 
Solution. 

Wt.  of  i  cc. 
Solution. 

Gms.  CioHg 
per  100  Gms. 
C6H5.CH3. 

-50 

o-3 

—  20 

1.9 

O 

5-5 

0.9124 

+  10 

27-5 

24.0 

9.0 

0.9126 

15.0 

20 

36.0 

31.0 

14.0 

0-9*35 

28.0 

25 

40-5 

35-o 

J7-5 

0-9I55 

36.0 

30 

45-5 

39-o 

21  .O 

0.9180 

42  -O 

40 

54-o 

48.0 

30.8 

0.9250 

56.0 

50 

65.0 

57-5 

43-7 

0-935° 

69-5 

60 

77-5 

7o-5 

60.6 

0-9475 

83.0 

70 

88.0 

85.0 

78.8 

o  .  9640 

97-5 

80 

0.9770 

in  .0 

NAPHTHOIC    ACID    C10H7COOH. 
One  liter  of  aqueous  solution  contains   0.058  gram  C10H7COOH  at 

J°.  (Paul  — Z.  physik.  Ch.  14,  m,  '94.) 


/3  NAPHTHOL  208 

/3  NAPHTHOL    C10H7OH. 

100  grams  H2O  dissolve  0.105  gram  at  25°,  and  1.33  grams  at  b.  pt.; 
100  grams  alcohol  dissolve  164.0  grams  at  25°. 

NARCEINE. 

100  grams  pure  carbon  tetra  chloride  dissolve  o.on  gram  narceine 

at  17°.  (Schindelmeiser  —  Chem.-Ztg.  25,  129, '01.) 

NEODYMIUM    CHLORIDE    NdCl3. 

100  grams  H2O  dissolve  98.7  grams  NdCl3at  13°,  and  140. 4  grams  at 

I OO°.  (Matignon  —  Compt.  rend.  133,  289,  '01  ) 

NEODYMIUM    SULPHATE    Nd2(SO4)3. 

SOLUBILITY  IN  WATER. 

(Muthmann  and  Rolig  —  Ber.  31,  1728,  '98.) 

0         Gms.  Nd2(SO4)3  per  100  Gms.  Gms.  Nd2(SOj)3  per  100  Gms. 

Solution.     *       Water.  Solution.  Water. 

o  8.7  9.5  50  3.5  3.7 

16  6.6  7.1  80  2.6  2.7 

30  4-7  5-o  Io8  2-2  2-3 

NICKEL    BROMATE    Ni(BrO3)2.6H2O. 

100  grams  cold  water  dissolve  27.6  grams  nickel  bromate. 

NICKEL    BROMIDE    NiBr,. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  539,  '94-) 

t  o  Gms.  NiBr2  per 

100  Gms.  Solution, 

80  60.6 

100  60 . 8 

120  60.9 

140  61 .o 


NICKEL    CHLORATE    Ni(ClO3)2. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  35,  1419,  '02.) 

Gms.            Mols.                                                             Gms.  Mols. 

+  o        Ni(ClO3)2     Ni(ClO3)2           Solid                    t  o           Ni(ClO3)2  Ni(ClO3)2            Solid 

'      per  too  Gms.     per  100            Phase.                                penooGms.  per  100            Phase. 

Solution.    Mols.H2O.                                                   Solution.  Mols.H2O. 

— 18    49-55    7^4  Ni(ClO3)2.6H2O     48     67.60  16.65  Ni(ClO3)2.4H2O 

-  8      51.52      8.49           "                55        68.78  17.59 

o      52.66      8.88           "                65        69.05  18.01 

+  18      56.74    10.47           "                79-5     75-5°  24-68 

40      64.47     15-35            "             -13-5    3I-85  3-73          Ice 

—  9        26.62  2.90 

Sp.  Gr.  of  solution  saturated  at  +  18  =  1.661. 


-o         G     ms.NiBr2per             f0          Gms.  NiBr2  per 
1  *         100  Gms.  Solution.                      100  Gms.  Solution. 

—  20 
—  10 

47-7 
50-5 

25 
30 

57-3 
58.0 

O 
+  10 
2O 

53-o 
55-o 
56.7 

40 
60 

60.0 
60.4 

20Q 


NICKEL    CHLORIDE 


NICKEL    CHLORIDE    NiCl2. 

SOLUBILITY  IN  WATER. 

(Etard;  at  12°,  Ditte  —  Compt.  rend.  92,  242,  '81.) 


t°. 

Gms.  NiCl2  per 
100  Gms.  Solution. 

t    . 

Gms.  NiCI2  per 
100  Gms.  Solution. 

t°. 

Gms.  NiCl2  per 
loo  Gms.  Solution. 

-17 

29.7 

25 

4O.O 

60 

45-i 

o 

35-o 

30 

40.8 

70 

46.0 

+  10 

37-3 

40 

42-3 

78 

46.6 

20 

39-i 

So 

43-9 

100 

46.7 

1000  cc.  sat.  HC1  solution  dissolve  4.0  grams  NiCl2  at  12°. 
100  grams  abs.  alcohol  dissolve  53.71   grams  NiCl2.6H2O  at  room 
temperature. 

100  grams  abs.  alcohol  dissolve  10.05  grams  NiCl2 at  room  temperature. 

(Bodtkcr —  Z.  physik.  Chem.  22,  511,  '97.) 

ioo  grams  abs.  alcohol  dissolve  2.16  grams  NiCl2.7H2O  at  17°,  and 


1.4  grams  at  3 


(de  Bruyn  —  Rec.  trav.  chim.  n,  156,  '92.) 


ioo  grams  saturated  solution  in  glycol  contain  16.2  grams  NiCl2  at 

room  temperature.  (de  Coninck  —  Bui.  acad.  roy.  Belgique,  359,  '05.) 


NICKEL    IODATE 


Gms. 

Mols. 

t°. 

Ni(I03)2 
per  ioo  Gms. 

Ni(I03)2 
per  ioo  Mols. 

Solution. 

H2O. 

O 

o-73 

0-033 

18 

1  .01 

0-045 

30 

1.41 

0.063 

0 

o-53 

0.023 

18 

0.68 

0.030 

30 

0.86 

0-039 

50 

1.78 

O-o8o 

8 

0.52 

0.023 

Ni(I03)2. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  34,  2440,  '01.) 


Solid 
Phase. 


Ni(I03)24H20 


Ni(IO3)2.2H2O  (i) 


Ni(I03)2.2H20  (2) 


(i)   a  Dihydrate. 


Gms. 
to        Ni(I03)2 
'   per  ioo  Gms 
Solution. 

Mols. 
Ni(IO3)2               Solid 
.  per  ioo  Mols.         Phase. 
H20. 

18 
5o 

o-55 
0.81 

0  .  0245     Ni(IO3)2.2H2O  (2) 
0-035 

75 
80 

1.03 

I  .12 

0-045 
0.049 

30 

I-I35 
1.07 

0  .  050        Ni(IO3)2 

o  -  046 

75 

I  .02 

0-045 

90 

0.988 

0-044 

(2)  0  Dihydrate. 


NICKEL    IODIDE 


—  20 

o 

10 

20 


Gms.  NiI2  per 
ioo  Gms.  Solution. 

52.0 

55-4 
57-5 
59-7 


NiI2. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  546,  '94.) 

ioo  Vjms.  aoiuuon. 

60 
70 
80 
90 


25 
30 
40 


Gms.  NiI2  per 
ioo  Gms.  Solution. 

60.7 
6l.7 

63-5 
64.7 


Gms.  NiI2  per 
ioo  Gms.  Solution. 

64.8 
65.0 

65.2 
65-3 


KICKEL    NITRATE 


210 


NICKEL    NITRATE    Ni(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt,  3,  439,  'oo.) 


Gms.  Mols. 

to          Ni(N03)2      Ni(N03)2 

per  100  Gms.  per  100  Mols. 


Solid 
Phase. 


Solution. 

H20. 

-23 

39-02 

6.31 

—  21 

39-48 

6-43 

-10-5 

44-13 

7-79 

—  21 

39-94 

6-55 

-12.5 

41-59 

7.01 

—  10 

42.11 

7.16 

-  6 

43.00 

7-44 

0 

44  -32 

7.86 

+  18 

48-59 

9-3 

Ni(N03)2.9H20 


Ni(NO3)2.6H2O 


Gms.  Mols. 

to         Ni(N03)2      Ni(N03)2  Solid 

'    per  100  Gms.  per  100  Mols.        Phase. 
Solution.          H2O. 


Ni(N03)2.6H2O 


Ni(N03)3.3H20 


20 

49-06 

9-49 

4i 

55-22 

12  .1 

56-7 

62.76 

I6.7 

58 

61.61 

15-9 

60 

61.99 

16.0 

64 

62.76 

16.6 

70 

63-95 

17.6 

90 

70.16 

23.1 

95 

77.12 

33-3 

100   grams   sat.   solution   in  glycol  contain  7.5  grams  Ni(NO3)  at 
room  temperature.  (de  Coninck.) 


NICKEL    SULPHATE    NiSO4. 

SOLUBILITY  IN  WATER. 

(Steele  and  Johnson  —  J.  Ch.  Soc.  85,  116,  '04;  see  also  Etard  and  Mulder.) 


Grams  NiSO4  per                                                             Grams  NiSO4  per 
t°.                    100  Gms.                      5«j«                        to                    TOO  Gms. 

Solid 

T>U     ~ 

Solution.      Water.                                                         Solution.       Water." 

.rnase* 

5            20-47       25.74      NiS04.7H20               33.0      30.25      43.35 

NiSO4.6H2O 

o        21.40    27.22                             35.6    30.45     43-79 

'      (blue) 

9        23.99    31.55                            44.7    32.45     48.05 

" 

22.6      27.48      37.90                                         50.0      33.39      50.15 

" 

30            29.99      42.46                                         53.0      34.38      52.34 

" 

32-3     30-57     44-02                               54.5     34.43     52.50 

NiSO4.6H20 

33        3J-38     45-74            "                57  -o    34-8i     53.40 

"    (green) 

34        31-20    45-5                               60        35.43     54.80 

" 

32-3    30-35     43-57     Niso4.6H2o          70        37.29    59.44 

M 

33-o    30-25     43-35            "    <blue>      80        38.71     63.17 

H 

34-o    30.49     43-83                             99        43-42     76-71 

" 

Transition  points,  hepta  hydrate  <=±  hexa  hydrate  =31 
Hexa  hydrate  (blue)  «=>  hexa  hydrate  (green)  =  53.3°. 

•5°. 

211 


NICKEL    SULPHATE 


SOLUBILITY  OF  MIXTURES  OF  NICKEL  SULPHATE  AND  COPPER  SULPHATE. 


Results  at  35°. 


(Fock  —  Z.  Kryst.  Min.  28,  387,  '9?-) 


Gms.  per  100  Gms.  H;jO. 

Hol.  per  cent  in  Solution.     I 

dol.  per  cent  in  Solid  P 

hase.       Crystal 

CuSO4.        NiSO4. 

'CuS04.          NiS04." 

CuSO4.        NiSO4.  '             Form. 

9.62       583.9 

i-57     98.43 

°-35       99-65           Rhombic 

41.66      484.4 

7.69     92.31 

2.12     97.8 

3 

75-39    553-5 

11.66     88.34 

4-77        95-23            Tetragonal 

106.40    506.5 

16.92     83.08 

6.52       93.48 

172.0      483-8 

25-63      74-37 

13.88       86.17 

186.9      468.0 

27.90     72.10 

l8  .77       8l  .  23            Tetragonal 
94.91           5-O9            Triclinic 

Results  at  67°. 

20.04     729-3 

2-65     97-35 

0.93      99.07            Monoclinic 

66.01     706.2 

8.31     91.69 

2.86     97.14 

88.08     501.6 

13-55     86.45 

3.92      96.08 

47-94     675.0 

16.39     83.61 

6.66     93.34 

249.9       747-8 

24-46     75-54 

•?•?    •29       Ti    f\R         /Monoclinic 
•"•3-^       77  >uc          (Triclinic 

SOLUBILITY  OF  MIXTURES  OF  NICKEL 

SULPHATE  AND  SODIUM  SUL- 

PHATE,    ETC 

. 

(Koppel;  Wetzel  —  Z.  physik.  Chem.  52,  401,  '05.) 

Gms.  per  100 

Gms.  per  100 

Mols.  per  100 

t°.                Gms.  Solution. 

Gms.  H2O. 

Mols.  H20. 

Solid 

NiSO4.        Na2SO4. 

NiSO4.         Na2SO4. 

NiSO4.      Na2SO4.   " 

Phase  . 

o         16.94       7.61 

22.46       IO.O9 

2.61       1.28   ' 

5        17.99     10.85 

25.28       15-24 

2-94       i-93 

NiSO4.7H2O  + 
Na2SO4.ioH2O 

10        18.97     13.85 

28.26       20.64 

3.29       2.61 

20            18.76       17.21 

29.31       26.87 

3.410    3.404 

NiNa2(SO4)2.4H20 

25             17.85       16.54 

27-33       25.33 

3.181     3.208 

» 

30            16.74       15.34 

24.64       22.58 

2.868     2.861 

« 

35        16.28     14.91 

23.66       21.67 

2-753     2.744 

«« 

4o         15-35     J4-49 

21.88     20.65 

2.546     2.616 

«« 

18.5     19.61     16.49 

30.70    25.80 

3-56      3-27   * 

20        20.13     16.15 

3J-59     25.35 

3.67       3.21 

25             21.20       14.77 

33.11     23.06 

3.85       2.92 

NiNa2(SO4)2.4H20  -f 

30            22.60       I  2.  80 

34.98     19.82 

4.07       2.59 

NiSO4-7H2O 

35        23.62     10.78 

36.01     16.43 

4.19       2.08 

40        24.92      9.39 

37.93     14-29 

4.41       1.81    - 

18.5     16.80     18.93 

26.14     29.45 

3.04      3-72   ' 

20            15.48       20.  l8 

25         10.92     24.12 

24.06    31.37 
16.81     37.13 

2.80      3.97 
1.96      4.70 

NiNa2(S04)2.4H2O  4 
'      Na2S04.ioH20 

30         6.40    28.71 

9.87     44.25 

1.15       5.60  J 

35          4-54    31-65 

7-i3     49-59 

0.838     6.28 

NiNa2(S04)2.4H20  + 

40          4-63     31.37 

7.24    49.03 

o  .  843     6.21 

Na2SO4 

NICKEL    SULPHATE  212 

SOLUBILITY   OF   NICKEL   POTASSIUM    SULPHATE    NiK2(SO4)2.6H2O    IN 

WATER. 

(Tobler  —  Liebig's  Ann.  95.  193.  'SSJ  v.  Hauer  — J.  pr.  Ch.  74,  433,  '58.) 

Grams  NiK2(SO4)2  Grams  NiK2(SO4)2 

*o  per  TOO  Gms.  H2O.  ^0  per  100  Gms.  H^. 

'  (Tobler.)     (v.  Hauer.)"  '  (Tobler.)     (v.  Hauer.)' 

05-3  50       30 

10      8.9      ...        60     35.4     20.47 

20        13.8         9.53          70        42.0 

30     18.6      ...       80     46.0     28.2 

40        24-0        I4-03 


SOLUBILITY  OF  NICKEL  SULPHATE  IN  METHYL  AND  ETHYL  ALCOHOLS. 

(de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '92.) 

ioo  grams  abs.  ethyl  alcohol  dissolve  1.3  grains  NiSO4.7H2O  at  17°. 

100  grams  abs.  methyl  alcohol  dissolve  46.0  grams  NiSO4.7H2O  at 
17°,  and  24.7  grams  at  4°. 

ioo  grams  abs.  methyl  alcohol  dissolve  0.5  gram  NiSO4  at  18°. 

ioo  grams  abs.  methyl  alcohol  dissolve  31.6  grams  NiSO4.6H2O  at  17°. 

ioo  grams  93.5%  methyl  alcohol  dissolve  10.1  grams  NiSO4>7H2O  at 
4°,  and  7.8  grams  NiSO4.6H2O  at  18°. 

ioo  grams  50.0%  methyl  alcohol  dissolve  2.0  grams  NiSO4.7H2O  at 
4°,  and  1.9  grams  NiSO4.6H2O  at  18°. 

ioo  grams  sat.  solution  in  glycol  contain  9.7  grams  NiSO4  at  room 
temperature. 

(de  Coninck  —  Bull.  acad.  roy.  Belgique  359,  '05.) 


NICOTINE    C10H14N2. 

SOLUBILITY  IN  WATER. 

(Hudson  —  Z.  physik.  Chem.  47,  114,  '04.) 

Determinations  made  by  Synthetic  Method,  for  which  see  Note,  page 
9.  Below  60°  and  above  210°  both  liquids  are  miscible  in  all  propor- 
tions; likewise  with  percentages  of  nicotine  less  than  6.8  and  above  82 
per  cent  the  liquid  does  not  show  two  layers  at  any  temperature. 
Below  94°  the  upper  layer  is  water.  Above  94°  the  upper  layer  is 
nicotine.  The  curve  plotted  from  the  following  results  makes  a  com- 
plete circle. 


in 

6.8  94  95 

7-8  89  155 

10.  o  75 

14.8  65  200 

32.2  61  210 

49-0  64  205 

66.8  72  190 

80.2  87  170. 

82,0  129  130 


213  NITROGEN 

NITROGEN    N. 

SOLUBILITY  IN  WATER. 

(Winkler  —  Ber.  24,  3606,  '91;  Braun  — Z.  physik.  Chem.  33,  732,  'oo;  Bohr  and  Bock  —  Wied.  Ann. 

44,  318,  '0i.) 


O 

0.0235* 

o.o239t 

...J 

0.0233* 

0.00239* 

5 

0-0208 

0.0215 

0.0217 

0.0206 

0.00259 

10 

0.0186 

0.0196 

0-0200 

0.0183 

0.00230 

15 

0.0168 

0.0179 

0.0179 

0.0165 

0.00208 

20 

0.0154 

0-0164 

0.0162 

0.0151 

0.00189 

25 

0.0143 

0.0150 

0.0143 

0.0139 

0.00174 

30 

0.0134 

0.0138 

0.0128 

o.  00161 

35 

0-0125 

0.0127 

0.0118 

0.00148 

40 

0.0118 

0.0118 

O-OIIO 

0.00139 

5° 

0.0109 

0.0106 

.  .  . 

0.0096 

O.OOI2I 

60 

O-OIO2 

o.oioo 

0.0082 

0.00105 

80 

0.0096 

0.0051 

0.00069 

IOO 

0.0095 

o.oioo 

o.oooo 

o.ooooo 

*W.  fB.andB.  $  B. 

For  values  of  ft,  ft',  and  q,  see  Ethane,  page  133. 

SOLUBILITY  OF  NITROGEN  IN  AQUEOUS  SALT  SOLUTIONS. 

(Braun.) 
Coefficient  of  Absorption  of  N  in  Barium  Chloride  Solutions  of: 


t°. 

13-83 

11.92 

6.90 

3-87 

3-33 

per  cent. 

per  cent. 

per  cent. 

per  cent. 

per  cent. 

5 

0.0127 

0.0137 

0.0160 

O-OlSo 

0-0183 

10 

O.OII7 

0.0125 

O.OI47 

0.0166 

o.oies 

15 

O-OIO4 

O-OII4 

0.0132 

0.0148 

0.0150 

20 

0.0092 

0.0098 

0.0118 

0.0132 

0.0135 

25 

0.0078 

0.0086 

0.0104 

O.OII4 

O.OII9 

Coefficient  of  Absorption  of  N  in  Sodium  Chloride  Solutions  of: 


t°. 

11-73 

8.14 

6.4 

2.12 

0.67 

per  cent. 

per  cent. 

per  cent. 

per  cent. 

per  cent. 

5 

O-OIO2 

O.OI27 

0-0138 

O.OI79 

0-02OO 

10 

0.0093 

O.OII3 

O.OI26 

0.0164 

0.0185 

i.S 

O.OoSl 

O-OIOI 

O.OII3 

O.OI47 

0.0164 

20 

O.O066 

0.0087 

0-0098 

O.OI3I 

0-0148 

25 

0-0047 

0.0075 

0.0083 

O.OH3 

O.OI3O 

SOLUBILITY  OF  NITROGEN  IN  ALCOHOL. 

(Bunsen.) 
t°  0°  5°  10°  15°  20°  24° 

Vols.  N  *  0.1263     0.1244     0.1228     0.1214     0.1204     0.1198 

dissolved  by  i  Vol.  Alcohol. 

*  At  o°  and  760  mm. 


NITROGEN 


214 


SOLUBILITY   OF   NITROGEN   IN   MIXTURES   OP  ALCOHOL  AND  WATER 

AT  25°. 

(Just  —  Z.  physik.  Ch.  37,  361,  '01.) 

Results  in  terms  of  the  Ostwald  solubility  expression,  see  page  105. 

Vol.  H2O  in  Mixture.    Vol.  Alcohol  in  Mixture.  Dissolved  N  (/2s). 

ioo          o  0.01634 

80  20  0-01536 

67  33  0.01719 

o  ioo  (99 . 8  %  Alcohol)  o .  1 43  2 


SOLUBILITY  OF  NITROGEN  IN  SEVERAL  SOLVENTS  AT  20°  AND  25°. 

(Just.) 

Solvent.                             /25.  ISQ. 

Toluene  0.1235  0.1186 

Chloroform  0.1348  0.1282 

Methyl  Alcohol  o.  1415  o.  1348 

Ethyl  Alcohol  (99.8%)  o.  1432  o.  1400 

Acetone  o.  1460  o.  1383 

Amyl  Acetate  o.  1542  o.  1512 

Ethyl  Acetate  0.1727  0.1678 

Iso  Butyl  Acetate  0.1734  0.1701 


Solvent. 

I2b. 

feo. 

Water 

0.01634 

0.01705 

Aniline 

0.03074 

0.02992 

Sulphur  Dioxide 

0.05860 

0.05290 

Nitro  Benzene 

0.06255 

0.06082 

Benzene 

0.1159 

o.  1114 

Acetic  Acid 

o.  1190 

o.  1172 

Xylene 

0.1217 

0.1185 

Amyl  Alcohol 

o.  1225 

o.  1208 

SOLUBILITY  OF  NITROGEN  IN  PETROLEUM.   COEFFICIENT  OF  ABSORP- 
TION   AT    10°    =  0.135,    AT    20°    =   O.II7. 
(Gniewasz  and  Walfisz  — Z.  physik.  Ch.  i,  70,  '87  ) 


SOLUBILITY  OF   NITROGEN  IN  AQUEOUS   PROPIONIC  ACID  AND  UREA 

SOLUTIONS. 

(Braun.) 
Coefficient  of  Absorption  of  N  in  C2H5COOH  Solutions  of: 


tl    . 

11.22  per  cent. 

9.54  per  cent. 

6.07  per  cent. 

4.08  per  cent. 

3.82  per  cent. 

5 

10 

IS 

20 

0.0195 
0.0178 
0.0159 
0.0146 

0.0204 
0.0l82 
0.0163 
0.0147 

0.0208 

0.0186 

0-0164 
0-0148 

O.O2IO 
0.0192 
0.0169 
O.OI54 

O.0209 
O.OI9I 
0.0l67 
0.0155 

25 

O.OI3O 

0.0134 

0.0134 

0.0137 

0.0137 

Coefficient  of  Absorption  of  N  in  CO(NH2)2  Solutions  of: 


V      . 

15.65  percent. 

1  1.  9  per  cent. 

9.42  percent. 

6.90  per  cent. 

5.15  per  cent. 

2.  28  per  cent. 

5 

10 

TS 

20 

0.0175 
O.Ol62 
O.OI5O 
O.OI4O 

0.0179 
0.0167 
0-OI49 
0.0139 

O.OI9O 
0.0176 
0.0158 
O.OI46 

0.0198 
0-0183 
0.0165 
O.OI5I 

O.OI97 
0.0l82 
0.0165 
O.OI5I 

O.OI99 
0.0184 
O.OI7I 
0.0155 

25 

O.OI3O 

O.OI30 

0.0133 

0.0137 

0.0135 

0.0139 

215  NITROUS    OXIDE 

NITROUS    OXIDE    N2O. 

SOLUBILITY  IN  WATER. 

(Bunsen;  Gordon  —  Z.  physik.  Ch.  18,  9,  '95;  Roth — Ibid.  24,123,  '97;  Knopp  —  Ibid.  48,106,  '04 
Geffcken — Ibid.  49,  276,  '04.) 


*°. 

(B.) 

(G.) 

(R) 

(K.) 

q 

'(R.) 

5 

1.0950 

1-0955 

i  .  1403 

o  .205 

i  .  161 

10 

0.9196 

o  .9200 

0.9479 

o  .  171 

0.9815 

15 

0.7778 

0.7787 

0.7896 

0.143 

0  -8315 

20 

0.6700 

o  .6700 

0.6654 

o  .6270 

0.  121 

o  7131 

25 

0.5961 

0-5752 

o.  104 

0.6281 

Coefficient  of  Absorption  /3.  */-»^UM^y  m  te-rms/(N 

of  Ostwald  Expression  (/).* 

K-.)  (0? 

I  .067 
.  .       o .9101 

0.7784 

739     0-6756 
0.5992 
*  Calculated  by  Geffcken. 

NOTE.  —  Knopp  and  also  Geffcken  call  attention  to  the  fact  that 
Roth  in  making  his  determinations  used  a  rubber  tube  between  the 
gas  burette  and  the  shaking  flask,  and  give  this  as  an  explanation  of 
the  high  results  which  he  obtained. 


SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SULPHURIC  ACID. 

(Lunge  —  Ber.  14,  2188,  '81;  see  also  Geffcken 's  results.) 

Sp.  Gr.  of  H2SO4  1.84          i. 80          I-7o5  i-45  1-25 

Vols.  N2O  dissolved 

by  100  vols.  H2SO4         75.7          66.0          39.1  41.6          33.0 


100  vols.  of  KOH  solution  of  1.12  Sp.  Gr.  absorb  18.7  vols.  N2O. 
100  vols.  of  NaOH  solution  of  i.io  Sp.  Gr.  absorb  23.1  vols.  N2O. 

SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OF  ACIDS. 

(Geffcken.) 

Results  in  terms  of  the  Ostwald  Solubility  Expression  (/).    See  p.  105, 
In  Hydrochloric  Acid.       In  Nitric  Acid.          In  Sulphuric  Acid. 

Cms.  HCl 
per  Liter. 

l8.22 

36-45 
72.90 


SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OF: 

(Roth.) 

Phosphoric  Acid.  Oxalic  Acid. 


N2O  Dissolved 

Gms.HNOa    N20  Dissolved 

Gms.  H2SO4    1 

ST2O  Dissolved 

/«• 

/25- 

per  Liter. 

la- 

/25- 

per  Liter. 

/15- 

ks- 

'-755 

0. 

577 

36. 

52 

0.777 

0-597 

24.52 

o. 

734 

O. 

566 

'.738 

o. 

568 

63- 

05 

0.777 

0.602 

49-04 

0. 

699 

0 

•543 

).  716 

o, 

•557 

126. 

IO 

0-775 

0.611 

98.08 

o. 

645 

0 

509 

147.12 

0. 

602 

o. 

482 

196.  16 

0. 

562 

0. 

463 

t° 
5 

10 

15 
20 

25 

Coefficient  of  Abs.  in  H3PO4  Solutions  of: 

-* 

Coefficient  of  Abs.  in 
(COOH)2  Solutions  of: 

3-38%. 

1-057 
0.8827 
0-7388 
0.6253 
0.5427 

4-72%. 

I  -0365 
0.8665 
0.7258 
0.6147 
0-5329 

8.84%. 
0.9883 
0-8296 
0.6977 
0.5926 
0.5143 

9.89%. 

o-9635 
0.8101 
0.6826 
0.5810 
0-5054 

13-35%. 
0.9171 
0.7711 
0.6505 

o-5555 
o  .  4860 

0.812%. 
I.I450 
0.9526 
0.7940 
0.6694 
0.5784 

3-70%. 
I.I094 
0.9264 

0-7745 
0.6538 
0-5643 

NITROUS    OXIDE 


216 


SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OF  PROPIONIC 

ACID  AT  20°. 

(Knopp.) 

Gms.  C2H5COOH 

per  liter  ^S-^S         60.42         158.4  176.6          344-° 

Coef.  of  Absorp- 
tion of  N2O  0.6323      0.6369        0.6504        0.6534        0.7219 


SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SALT  SOLUTIONS. 


Results  by  Geffcken  in  terms 
page  105. 

Salt. 

Ammonium  Chloride 
Ammonium  Chloride 
Caesium  Chloride 
Lithium  Chloride 
Lithium  Chloride 
Potassium  Bromide 
Potassium  Bromide 
Potassium  Chloride 
Potassium  Chloride 
Potassium  Iodide 
Potassium  Iodide 
Potassium  Hydroxide 
Potassium  Hydroxide 
Rubidium  Chloride 
Rubidium  Chloride 


of  the  Ostwald  expression  (/).      See 


Cone,  of 

Salt  per  Liter. 

Solubility 

of  N2O. 

Formula,, 

Gram  Equ 

iv.      Grams. 

*i*. 

'*. 

NH4C1 

o-5 

26.76 

0.730 

o-557 

NH4C1 

I  .0 

53-52 

0.691 

0.529 

CsCl 

o-5 

84.17 

O.7IO 

0-544 

LiCl 

o-5 

21  .24 

0.697 

o-535 

LiCl 

I  .0 

42.48 

0.623 

0.483 

KBr 

o-5 

59-55 

0.697 

0-536 

KBr 

I  .0 

119.11 

0.627 

0.485 

KC1 

o-5 

37-3 

0.686 

0.527 

KC1 

I  .0 

74-6 

0.616 

o-475 

KI 

o-5, 

83.06 

0.702 

0.541 

KI 

I  .0 

166.12 

0-633 

0.492 

KOH 

o-5 

28.08 

0.668 

0.514 

KOH 

i  .0 

56.16 

o-559 

0.436 

RbCl 

o-5 

60.47 

0.695 

0-533 

RbCl 

I  .0 

120.95 

0.625 

0.483 

Results  by  Knopp,  in  terms  of  the  coefficient  of  absorption,,     See 


page  105. 


Salt. 


Formula. 


Potassium  Nitrate     KNOq 


Sodium  Nitrate 


NaNOq 


Cone,  of  S; 

lit  per  Liter. 

Coef.  of  Absorption 

Normality. 

Grams. 

of  N20  at  20°. 

0.1061 

10-74 

0-6173 

0.2764 

27.94 

o  .  6002 

0.5630 

56-97 

0-57*3 

1.1683 

118.2 

0:5196 

0.1336 

"•37 

o  .  6089 

0.3052 

25-97 

0.5876 

0.6286 

53-5o 

0-5465 

i  .1200 

95-30 

0.4926 

Results  by  Roth,  in  terms  of  the  coefficient  of  absorption. 


Grams  NaCl  per 
100  Grams 
Solution. 

0.99 
1.  808 

7.886 
5-865 

Coefficient  of  Absorption  of  N2O  at: 

5°. 
I  .0609 
I    OO32 
0-9131 
0.8428 

10°.                     15°.                        20°. 

0.8812        0.7339        0.6191 
0.8383        0.7026        0.5962 
0.7699        0.6495        0.5520 
0.7090        0.5976        0.5088 

25°. 

0.5363 
0.5190 

0.4475 
0.4224 

217  NITROUS    OXIDE 

SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SALT  SOLUTIONS. 
Results  by  Gordon  in  terms  of  coefficient  of  absorption.    See  p.  105. 

Concentration  of  Salt.  Coefficient  of  Absorption  of  N2O  at: 


Salt.                            Grams  per         Gram 
100  Grams         Mols.                         5°. 
Solution.       per  Liter. 

10°. 

15°. 

20° 

Calcium  Chloride          5  .  79 

o-547 

0.819 

0.697 

0.591 

0.500 

9.86 

0.964- 

0.668 

0.586 

0.509 

0 

•435 

13-99 

i  .416 

0.510 

0.441 

0-380 

0 

.328 

Lithium  Chloride          1.35    . 

0.319 

0.986 

0.831 

O.7OO 

0 

•594 

3  -.85 

0.928 

0.878 

0-743 

O.O29 

0 

•536 

11.48 

2.883 

0.606 

0.512 

o-437 

0 

.382 

Lithium  Sulphate          2.37 

0.219 

0-934 

0.792 

0.670 

0 

•569 

5-46 

0.521 

o-795 

0.665 

o-557 

0 

•474 

8.56 

0.836 

0.646 

o-555 

o-477 

0 

•415 

Magnesium  Sulphate    5  .  90 

0.521 

0.766 

0.664 

0.561 

0 

.471 

7.66 

0.687 

0.708 

0.586 

0.488 

0 

.414 

10.78 

o-997 

0.569 

0.491 

0.417 

0 

•346 

Potassium  Chloride      4-90 

0.676 

0.879 

0-751 

0.643 

0 

•555 

7.64 

1.037 

0-799 

0-693 

0.591 

0 

•494 

14-58 

2.147 

0-654 

o-574 

0.500 

0 

•430 

22.08 

3-4I4 

Q-544 

0-459 

0-390 

0 

•339 

Potassium  Sulphate      2  .  62 

0.154 

0.986 

0-831 

0.701 

0 

.605 

4-78 

0.285 

0.918 

0.763 

0-637 

0 

•542 

Sodium  Chloride           6  .  20 

i  .107 

0.800 

0.682 

0-585 

0 

•509 

8.88 

i  .614 

0.713 

0.603 

0.510 

0 

•434 

12.78 

2.391 

0.634 

o-532 

0-449 

0 

.386 

Sodium  Sulphate           5  .  76 

0.427 

0.808 

0.677 

0.584 

0 

•495 

8-53 

0.646 

0.692 

o-574 

0.482 

0 

.416 

12.44 

Q-974 

0-559 

0-486 

0.417 

o 

•354 

Strontium  Chloride       3.31 

0.215 

0.928 

0.788 

0.671 

0 

•578 

5-73 

0.380 

0.848 

0.709 

0.610 

0 

•550 

13-24 

o-939 

0.644 

0-547 

0.463 

0 

.390 

SOLUBILITY  OF  NITROUS  OXIDE  IN  ALCOHOL  AND  IN  AQUEOUS  CHLORAL 

HYDRATE 

SOLUTIONS 

AT    20° 

. 

(Bunsen;  Knopp 

—  Z.  physik.  Ch. 

48,  1  06,  '04.) 

In  Alcohol  (B.). 

In  Aq 

.  Chloral  Hydrate  (K.). 

Vols.  N2O 

Normality 

Gms. 

r*~~t    ~t 

t  °.        (it  o°  and  760  mm.) 

of                  C2HC13O.H20           AI^'M.^ 

per  i  Vol  .  Alcohol  .       C2HC13O  .H2O  . 

per  Liter. 

2v-'» 

o             4-178 

0.184 

30-43 

0.618 

5            3-844 

0-445 

73.60 

0.613 

10            3.541 

0.942 

155-8 

0.596 

I5                  3.268 

I  .165 

192.7 

0-589 

20            3-025 

1-474 

243-8 

o-579 

24            2.853 

I  .911 

316.4 

0.567 

SOLUBILITY  OF  NITROUS  OXIDE  IN  PETROLEUM.     COEFFICIENT  OF 
ABSORPTION  AT   10°  =  2.49,  AT  20°  =  2.11. 

(Gniewasz  and  Walfisz  — Z.  physik.  Ch.  i,  70,  '87.) 


NITROUS    OXIDE 


218 


SOLUBILITY  OF  NITROUS  OXIDE  IN  AQUEOUS  SOLUTIONS  OF  GLYCERINE 

AND  OF  UREA. 

(Roth.) 
Coefficient  of  Absorption  of  N2O  in  Glycerine  Solutions  of: 


346  per  cent 

6.73  per  cent.       12 

.1  2 

per  cent.      16.24  per  cent. 

5 

i 

.097 

i 

•055 

0 

•999 

0 

•959 

10 

0 

.917 

0 

.887 

o 

.841 

0 

.810 

15 

0 

767 

0 

•745 

0 

.710 

0 

.686 

20 

o 

647 

0-630 

0 

.605 

0 

•585 

25 

0-556 

0 

•542 

0 

•527 

0 

-508 

Coefficient  of  Absorption  of  N2O  in 

Urea  Solutions  of: 

3^31 

per  cent 

4-97 

per  cent. 

6.37  per  cent. 

7.30  per  cent. 

9.97  per  cent. 

I 

.IO4 

I 

.096 

i  . 

088 

I  .101 

I  .069 

0 

.921 

O 

.920 

o. 

909 

0.921 

0.901 

0 

.771 

o 

•773 

o. 

76! 

0.772 

0.761 

0-653 

0 

.656 

o. 

644 

0-655 

0-651 

O 

•569 

o 

•567 

o. 

559 

0.570 

0-569 

Q. 

t°. 

ft. 

ft'. 

9. 

o  .  00984 

40 

0.0351 

0.0325 

0.00440 

o  .  00860 

50 

0.0315 

0.0277 

0.00376 

0.00757 

60 

0.0295 

0.0237 

0.00324 

o  .  00680 

70 

0.0281 

0.0195 

0.00267 

0.00618 

80 

0.0270 

0.0144 

0.00199 

0-00564 

90 

0-0265 

0.0082 

o  .00114 

0.00517 

100 

0.0263 

o.oooo 

o  .  ooooo 

t°. 

5 
10 

15 
20 

25 

NITRIC    OXIDE    NO. 

SOLUBILITY  IN  WATER. 

(Winkler  —  Ber.  34,  14*4,  '01.) 
t°.  ft.  ft'. 

o    0.0738     0.0734 

5    0.0646    0.0641 

10  0.0571  0-0564 

15  0-0515  0.0506 

2O  O.O47I  0.0460 

25  O.O43O  0-0419 

30  0.0400  0.0384 

For  values  of  ft,  ft'  and  q,  see  Ethane,  page  133. 

SOLUBILITY  OF  NITRIC  OXIDE  IN  AQUEOUS  SULPHURIC  ACID 
SOLUTIONS  AT  18°. 

(Lunge  —  Ber.  18,  1391,  '85;  Tower  —  Z.  anorg.  Ch.  50,  382,  '06.) 

Wt.  per  cent  H2SO4       Sp.  Gr. 
in  Solution.  at  15°. 

98  1.84 

90  1.82 

80  1.733 

70  1.616 

60  1.503 

5°  r-399 

*  Volume  of  NO  (at  760  mm.)  per  i  volume  of  aqueous  H2SO4. 

SOLUBILITY  OF  NITRIC  OXIDE  IN  ALCOHOL. 

(Bunsen.) 

t°  o°  5°  10°  15°          20° 

Vols.  NO*  0.316      0.300      0.286      0.275      0.266 

absorbed  by  i  vol.  Ale. 

*  At  o°  and  760  mm. 


Tension  of 
H2O  Vapor. 

Solubility  Coefficient  * 
of  NO  at  18°. 

0.0227        (0.035,  L.) 

o.i  mm. 

0-4      || 

0-0193 
O.OII7 

6.2       " 

O.OII3 
O.OIlS 
O.OI2O 

(0.017,  L. 

24" 
0.261 


2I9  OXALIC    AOID 

OXALIC    ACID    (COOH)2.2H2O. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Alluard;  Miczynski  —  Monatsh.  Ch.  7,  2158,  '86;  Henry  —  Com pt.  rend. 

99,  US?.  '84;  Lamouroux — Ibid.  128,  998,  'oo;  at  25°,  Foote  and  Andrew  — 

Am.  Ch.  J.  34,  154,  '05.) 

0  Grams  (COOH)2  per  roo  Grams  Grams  (COOH)^  per  100  Grams 

H2O.  Solution.  H2O.  Solution. 

o  3-45  3-33  40  21.15  17.46 

10  5-55  5-26  50  31-53  23-97 

20  8.78  8.07  60  45.55  3*-37 

25  11.36  10.21  70  63.82  38.95 

30  13.77  11.91 

SOLUBILITY  OF  OXALIC  ACID  IN  ALCOHOLS. 

(Timofeiew  —  Compt.  rend.  112,  1137,  '91;  Bourgoin  —  Ann.  chim.  phys.  [5]  13,  406,  '78). 

Grams  (COOH)2  per  100  Grams  of: 

t°.  , — ^- , 

Methyl  Alcohol.          Ethyl  Alcohol.          Propyl  Alcohol. 

-   i  36-26  20.25  9.73 

+  20  47-24  26.23  I5-I4 

SOLUBILITY  OF  OXALIC  ACID  IN  ABSOLUTE  AND  IN  AQ.  ETHER  AT  25°. 

(Bodtker —  Z.  physik.  Ch.  22,  512,  '97;  Bourgoin.) 

ioo  grams  absolute  ether  dissolve  1.47  grams  (COOH)2.2H2O. 
100  grams  absolute  ether  dissolve  23.59  grams  (COOH)2. 

In  Aqueous  Ether  Solutions. 

Gms.  Solid  Acid  Added  per  ioo  cc.  Ether  Solution.      Grams  per  ioo  cc.  Ether  Solution. 
(COOH)2.2H2O.      (COOH)2.  H20.  (COOH)2. 

(1)  5.0  o.o  I-25o  0.742 

(2)  5.0  o.o  0.788  0.720 
5.0              o.o                          0.418  1.044 

5.0  2.44  0.360  3.388 

5-0  4.82  0.484  6.038 

5-0  7.14  0.558  8.538 

5-0  9.42  0.632  10.996 

5.0  11.63  0.676  i3-3l6 

5.0  J3-79  0.761  15.684 

5.0  18.18  0.816  17.818 

5.0  22.73  0.816  17.818 

(i)  Ether  saturated  with  water.     (2)  Ether  containing  0.694  per  cent  water. 

ioo  grams  glycerine  dissolve  15  grams  oxalic  acid  at  15.5°. 
DISTRIBUTION  OF  OXALIC  ACID  BETWEEN  WATER  AND  AMYL  ALCOHOL 

AT    20°. 
(Herz  and  Fischer  —  Ber.  37,  4748,  '04.) 

Millimols  i(COOH)2  per  10  cc.  Grams  (COOH)2  per  ioo  cc. 


Aq.  Layer. 

\ 

Alcoholic  Layer. 

Aq.  Layer. 

Alcoholic  Layer. 

o.68c6 

O.I45I 

0.306 

0-0653 

2.364 

0.7233 

I  .064 

0.320 

6.699 

2-550 

3-015 

I.I48 

10.029 

4.300 

4-511 

1-934 

OXYGEN  220 

OXYGEN   O.  SOLUBILITY  IN  WATER. 

(Winkler  —  Ber.  24,  3609,  '91;  Bohr  and  Bock  —  Wied.  Ann.  [2]  44,  318,  '91.) 


t«.     Coef.  of  Absorption  ft.                 q. 

cc.  O  per         +o 
Liter  H*O. 

Coef.  of  Absorption  ft.               q. 

O 

O. 

0489* 

0.0496! 

0.00695 

10. 

187 

40 

0. 

0231* 

0.0233t 

0.00308 

5 

0. 

0429 

0.0439 

0.00607 

8. 

907 

5° 

O. 

O2O9 

0.0207 

0.00266 

10 

o. 

0380 

0.0390 

0.00537 

7- 

873 

60 

0. 

0195 

O.OlSg 

0.00227 

15 

0. 

0342 

0.0350 

0.00480 

7. 

038 

70 

o. 

0183 

0.0178 

0.00186 

20 

o. 

0310 

0.0317 

0.00434 

6. 

356 

80 

0. 

0176 

0.0172 

0.00138 

25 

0. 

0283 

0.0290 

0.00393 

5- 

776 

90 

o. 

0172 

0.0l69 

0.00079 

30 

o. 

0261 

0.0268 

0.00359 

5- 

255 

100 

0. 

0170 

0.0168 

o.ooooo 

*  w. 

t  B.  and 

B. 

For  values  of  /?  and  q  see  Ethane,  page  133. 

SOLUBILITY  OF  THE  OXYGEN  OF  AIR  IN  WATER. 
t°.  5.2°  5.65°  14.78°  24.8° 

Solubility  *  8  .  856  8  .  744  7  .  08  5.762 

*  cc.  Oxygen  per  1000  cc.  H2O  saturated  with  air  at  760  mm. 

SOLUBILITY  OF  OXYGEN  IN  WATER  AND  IN  AQUEOUS  SOLUTIONS  OF 
ACIDS,  BASES  AND  SALTS. 

(Geffcken  —  Z.  physik.  Ch.  49,  269,  '04.) 
Aq.  Solution  of:  Concentration  per  Liter.  Solubility  of  Oxygen* 

Water  alone 
Hydrochloric  Acid 


Nitric  Acid 

a 

(( 
Sulphuric  Acid 


Potassium  Hydroxide 

a 

Sodium  Hydroxide 

u 

Potassium  Sulphate 

u 

Sodium  Chloride 

u 


SOLUBILITY  OF  OXYGEN  IN  AQ.  POTASSIUM  CYANIDE  SOLUTIONS  AT  20°. 

(Maclaurin  —  J.  Ch.  Soc.  63,  737,  '93.) 

Cms.  KCN  per  100  gms.  sol.          i  10  20  30  50 

Coefficient  of  absorption  of  O     0.029      0.018      0.013       0.008      0.003 


Gram  Equiv, 

,    Grams. 

'    /16°. 

125. 

0.0363 

o  .  0308 

0.5 

18.22 

0.0344 

0.0296 

I  .0 

36-45 

0.0327 

0.0287 

2  .O 

72.90 

O.O299 

0.0267 

o-S 

36-52 

0.0348 

0.0302 

I  .0 

63-05 

0.0336 

0.0295 

2  .O 

126.10 

0-0315 

0.0284 

o-5 

24.52 

0-0338 

0.0288 

i.o 

49.04 

0.0319 

0.0275 

2.0 

98.08 

0-0335 

0.0251 

3.0 

147-12 

0.0256 

0.0229 

4.0 

196.16 

0.0233 

0.0209 

5-o 

245.20 

0.0231 

0.0194 

o-5 

28.08 

0.0291 

0.0252 

I  .0 

56.16 

0.0234 

0.0206 

o-S 

2O.O3 

0.0288 

0.0250 

I  .0 

40.06 

0.0231 

0.0204 

2.0 

80.  12 

O.OI52 

0.0133 

o-5 

43-59 

0.0294 

0*0253 

1  .0 

87.18 

0.0237 

0.0207 

o-5 

29.25 

0.0308 

0.0262 

I  .0 

58-5 

O.O26o 

0.0223 

2  .O 

119.0 

O.Ol82 

0.0158 

Dstwald  Solubi 

lity  Expressions 

.    See  page 

105. 

221  OXYGEN 

SOLUBILITY  OF  OXYGEN  IN  ETHYL  ALCOHOL,  METHYL  ALCOHOL  AND 

IN  ACETONE. 

(Timofejew —  Z.  physik.  Ch.  6,  151,  '90;  Levi  —  Gazz.  chim.  ital.  31,  II,  513,  '01.) 


In  Ethyl  Alcohol  of  99.7%  (T.). 

In  Methyl 
Alcohol  (L.) 

In  Acetone  (L.) 

/3. 

0'. 

0 

0-2337 

0.2297 

0.31864 

0-2997 

5 

O.230I 

0.2247 

0.30506 

0.2835 

IO 

o  .2266 

0.2194 

o  .  29005 

0.2667 

15 

0.2232 

0.2137 

0.27361 

o  .  2493 

20 

O.22OI 

0.2073 

0.25574 

0.2313 

25 

0.2177   (24°) 

0.2017   (24°) 

0.23642 

0.2127 

30 

0.21569 

0.1935 

40 

0.16990 

0-1533 

5° 

0.11840 

0.1057 

For  values  of  0  and  /3',  see  Ethane,  page  133.  /  =  Ostwald  Solu- 
bility Expression.  Seepage  105. 

The  formulae  expressing  the  solubility  of  oxygen  in  methyl  alcohol 
and  in  acetone  as  shown  in  the  above  table  are  as  follows: 

In  Methyl  Alcohol     /  =  0.31864  —  0.002572  t  —  o  00002866  t2. 
In  Acetone  /  =  0.2997     ~~  0-00318  t     —  0.000012  t2. 


SOLUBILITY  OF  OXYGEN  IN  AQUEOUS  ALCOHOL  AT  20°  AND  760  MM. 

(Lubarsch  —  Wied.  Ann.  [2]  37,  525,  '89.) 


Wt.  per  cent 
Alcohol. 

Vol.  per  cent 
Absorbed  O. 

Wt.  per  cent 
Alcohol. 

Vol.  per  cent 
Absorbed  O. 

Wt.  per  cent 
Alcohol. 

Vol.  per  cent 
Absorbed  O. 

o.oo 

9.09 
16.67 

2.98 
2.78 
2.63 

23-08 
28.57 

33-33 

2.52 
2.49 
2  .67 

50.O 
66.67 
8o.O 

3-50 

4-95 

5.66 

SOLUBILITY  OF  OXYGEN  IN  PETROLEUM.     COEFFICIENT  OF  ABSORP- 
TION AT    10°    =  0.229,    AT    20°    =  0.202. 
(Gniewasz  and  Walfisz  —  Z.  physik.  Ch.  i,  70,  '87.) 


OZONE    O,. 

SOLUBILITY  IN  WATER. 

(von  Mailfert  —  Compt.  rend.  119,  951,  '94;  Carius;  Schone  —  Ber.  6,  1224,  '73.) 
t°.  W.  G.  R.  t°.         W.  G,  R. 

o  39.4  61.5  0.641  27  13.9  51.4  0.270 

6  34.3  61.0  0.562  33  7.7  39.5  0.195 

1 1. 8  29.9  59.6  0.500  40  4-2  37-6  o.i 12 

13.0  28.0  58.1  0.482  47  2.4  31.2  0.077 

15-0  25.9  56.8  0.456  55  o-6  J9-3  0-031 

19.0  21 .o  55.2  0.381  60  o.o  12.3  o.ooo 

W  =  Milligrams  Ozone  dissolved  per  liter  water.  G  =  Milligrams 
Ozone  in  one  liter  of  the  gas  phase  above  the  solutions.  R  =  Ratio 
of  the  dissolved  to  undissolved  Ozone  (W  •*•  G) . 


PARAFFINE 


222 


SOLUBILITY  OP  OZOKERITE   PARAFFINE   OF  MELTING  POINT   64°-65° 
AND  SP.  GR.  AT  20°  =  0.917  IN  SEVERAL  SOLVENTS  AT  2O°. 


(Pawlewski  and  Filemonowicz  —  Ber.  21,  2973,  '88.) 


Gms.  Paraffine  per  100 


Solvent. 


Carbon  Bisulphide 
Benzine,  boiling  below  75 
Turpentine,  b.pt.  i58°-i66 
Cumol,  com.  b.pt.  160° 

"      frac.  150°-!  60° 
Xylene,  com.b.pt.  135°- 

"      frac.  i35°-i38° 
Toluene,  com.b.pt.io8°-iio° 

"       frac.  io8°-io9° 
Chloroform 
Benzene 
Ethyl  Ether 
Iso  Butyl  Alcohol,  com. 


Gms.  Paraffine  per  100 


Gms. 
Solvent. 

12.99 

cc. 
Solvent. 

Solvent. 
Acetone 

Gms. 
Solvent. 

O.  262 

cc. 

Solvent. 

o.  209 

'     n-73     8.48 

Ethyl  Acetate 

0.238 

.  .  . 

3° 

6.06 

5-21 

"     Alcohol 

o.  219 

4.26 

3-72 

Amyl  Alcohol 

0.  202 

o.  164 

3-99 

3-39 

Propionic  Acid 

o.  165 

o 

3-95 

3-43 

Propyl  Alcohol 

o.  141 

.  . 

4-39 

3-77 

Methyl  Alcohol 

o.  071 

0.056 

[0° 

3.88 

3-34 

Methyl  Formate 

o.  060 

.  .  . 

3-92 

Acetic  Acid 

o.  060 

0.063 

2.42 

3.1i 

"     Anhydride 

o.  025 

1.99 

Formic  Acid 

0.013 

0.015 

Ethyl  Alcohol  75% 

o.  0003 

0.285  0.228 


PAPAVERINE   C20H21NO4. 

100  grams  pure  carbon  tetra  chloride  dissolve  0.203  gram  at  17°. 

(Schindelmeiser  —  Chem.-Ztg.  25,  129,  Joi.) 


PHENANTHRENE   C14H10. 

SOLUBILITY  IN  ALCOHOL  AND  IN  TOLUENE.* 

(Speyers  —  Am.  J.  Sci.  [4]  14,  295,  '02.) 

In  Alcohol.  In  Toluene. 


t°. 

Gms.  CuHio  per 
100  Grams 

Sp.  Gr.  of 

Solutions 

Gms.  Ci4Hjo  per 
100  Grams 

Sp.  Gr.  of 
Solutions 

C2HSOH. 

(H20  at  4°.) 

C6H5.CH3 

(H20  at  4°.] 

0 

3-65 

0.814 

23.0 

0.925 

10 

3.80 

0.807 

30.0 

0.929 

20 

4-6 

O.Soi 

42.0 

0-934 

25 

5-5 

o-799 

50-0 

0-939 

30 

6.4 

o-797 

58.0 

Q-943 

40 

8.2 

o-795 

76.0 

0-955 

5° 

10.6 

0-794 

95-o 

0.971 

60 

IS  -6 

o-797 

115.0 

0.989 

7o 

33  -° 

0.815 

135  .0 

1.007 

80 

0.865  (76.4°) 

155.0 

i  .027 

*   Calculated  from  the  original  results  which  are  given  in  terms  of  gram  molecules  of  Phenanthrene 
per  100  gram  molecules  of  solvent,  and  for  irregular  intervals  of  temperature. 


Behrend  —  Z.   physik.    Ch.   10,    265,  '92,  finds  2.77  grams  phenan- 
threne  per  100  grams  alcohol  at  12.3°,  and  3.09  grams  at  14.8°. 


223  PHENANTHRENE 

SOLUBILITY  OF  PHENANTHRENE  PICRATE  IN  ABSOLUTE  ALCOHOL. 

(Behrend  —  Z.  physik.  Ch.  10,  205,  '92.) 

Grams  per  100  Grams  Saturated  Solution. 


Picric  Acid     +     Phenanthrene  =  Phenanthrene  Pi  crate. 
12-3  O.pl  0.71  1.62 

14.3  i.oo  0.78  1.78 

17.5  I.O5  O.82  1.87 

SOLUBILITY  OF   PHENANTHRENE    PICRATE   IN   ALCOHOLIC   SOLUTIONS 
CONTAINING  PICRIC  ACID  AND  ALSO  PHENANTHRENE. 

(Behrend.) 
Grams  Added  to  62  cc.  Abs.  Alcohol.  Cms.  per  100  Cms.  Sat.  Solution. 


P.  Picrate  +  Picric  Ac.  +  Phenanthrene. 

t  — 
Picric  Ac.  -f-  Phenanthrene 

=  P.  Picrate. 

12-3 

1-4 

0 

o-5 

0-534 

1-413 

1-947 

12-3 

1-4 

o 

0.9 

0.409 

2.141 

2-550 

12-3 

0.8 

o 

2  .1 

0-354 

2.77 

3-124 

I2.3 

0.8 

o 

4.0 

0-139 

5  .626 

5-765 

17-5 

1-4 

O.I 

0 

I-I59 

o-75 

I.9I 

17-5 

1.4 

0.2 

o 

1.285 

0.68 

1-97 

17-5 

1.4 

I  .0 

o 

2-45 

o-37 

2.82 

17-5 

1.4 

4.0 

0 

6.15 

o-i95 

6-345 

17-5 

1.4 

o.o 

2.2 

0.423 

3.276 

3-699 

PHENOL    C6H5OH. 

SOLUBILITY  IN   WATER. 

(Alexejew  —  Wied.  Ann.  28,  305,  '86;  Schreinemaker  —  Z.  physik.  Ch.  33,  79,  'oo;  Rothmund  —  Ibid 

26,  474,    98.) 

Determinations  were  made  by  the  "  Synthetic  Method,"  for  which 
see  Note,  page  9. 

Grams  Phenol  per  100  Grams 
Aqu 
10 
20 
30 
40 
50 

55 
60 

65 

68.3  (crit.  temp.)  33.4 

Vaubel  —  J.  pr.  Ch.  [2]  52,  73,  '95,  states  that  100  grams  sat.  aque- 
rus  solution  contain  6.1  grams  phenol  at  20°.  Sp.  Gr.  of  solution  = 
1.0057. 

SOLUBILITY  OF  PHENIC  ACID   (PHENOL,  C6H5OH)  IN  PARAFFINE 
AND  IN  BENZENE. 

(Schweissinger  —  Pharm.  Ztg.  '84- '85.) 

Grams  CeHsOH  per  100  Grams  Solvent  at: 

Solvent.  r- J 

16°.  21°.  25  .  43  • 

Paraffine  1.66  5.0 

Benzene  2.5  8.33  10.0  100.0 


Aqueous  Layer. 

Phenol 

Layer. 

7-5 

75 

.0 

8-3 

72 

.1 

8.8 

69 

.8 

9.6 

66 

•9 

12  .0 

62 

•7 

14-1 

59 

•5 

16.7 

55 

•4 

21.9 

49 

.2 

PHENOL 


224 


SOLUBILITY  OF  PHENOL  IN  AQUEOUS  ACETONE  SOLUTIONS. 

(Schreinemafcer .) 


In  4.24  % 
Acetone. 

Grams  Phenol  per 

In  12.2% 
Acetone. 

Gms.  Phenol  per 

In  24.4% 
Acetone. 

Gms.  Phenol  per 

In  59.9% 
Acetone. 

Gms.  Phenol  per 

t° 

ioo  Gms. 

ioo  Gms. 

ioo  Gms. 

ioo  Gms. 

L      . 

Aq  .  Acetone 
Layer. 

Phenol 
Layer. 

Aq  .  Acetone 
Layer. 

Phenol 
Layer. 

Aq  .  Acetone 
Layer. 

Phenol 
Layer. 

Aq.  Acetone 
Layer. 

Phenol 
Layer 

2O 

.  .  . 

.  .  . 

26.  0 

60.5 

3° 

5.0 

74.0 

4.0 

71.0 

6^0 

69-5 

28.5 

57-0 

40 

5-5 

70.0 

32.0 

52.0 

5° 

5-7 

67.  o 

5-° 

67.0 

8.0 

64.0 

34-  5§ 

49-  c§ 

60 

6-5 

61.0 

36.511 

46.511 

70 

9.0 

51.0 

7-5 

57-5 

19.  o 

57.0             (49-5°)  41-5 

80 

14  o 

34-o 

10.5 

49-5 

14.0 

52-5 

(84°)    22. 

5 

20.4* 

30-5* 

23.  ol 

47.  ot 

(90-  3°)  25 

c 

26.  si 

44.  oi 

(90-  5°)  35- 

0 

•90° 

t85° 

?87°.S 

§45° 

!l47°-S 

The  figures  in  the  above  table  were  read  from  curves  plotted  from 
the  original  results. 


SOLUBILITY  OF  PHENOL  IN  AQUEOUS  SOLUTIONS  d  TARTARIC  ACID. 

(Schreinemaker.) 


In  5.093%  Acid. 


In  19.34%  Acid. 


In  40.9%  Acid. 


Gms.  Phenol  per  ioo  Gms. 

Gms.  Phenol  per  ioo  Gms. 

Gms.PhenoIper  ioo  Gms. 

t°. 

Aq.  Acid 

Phenol 

t  . 

Aq.  Acid 

Phenol 

t  . 

Aq.  Acid 

Phenol 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

30 

7-5 

72-5 

5° 

10.  0 

77.0 

70 

I3.0 

50 

10.5 

65.5 

60 

12.5 

72.0 

80 

I6.5 

77.0 

60 

14-5 

58.0 

70 

19.0 

64.0 

85 

2O.  O 

74-o 

65 

19-5 

53-0 

75 

29.0 

56.0 

90 

26.5 

71.0 

67.5 

25.0 

48.5 

77 

47. 

,o 

95 

63.5 

69 

47-5 

97 

54. 

o 

DISTRIBUTION  OF  PHENOL  BETWEEN: 


AMYL  ALCOHOL  AND  WATER  AT  25°. 

(Herz  and  Fischer  —  Ber.  37,  4747,  '04.) 


Millimols  Phenol 
per  10  cc. 

Gms.  Phenol 
per  ioo  cc. 

Alcoholic  Aqueous 
Layer.     Layer. 

o.  75     o.  047 
0.9      0.05 
i.i       0.07 
2.6      o.  16 
54-1       3.83 
56.3      3-9 

Alcoholic  Aqueous 
Layer.      Layer. 

o.  705     o.  0441 
o.  846     o.  047 
1.035    0.066 
2.445    0.150 
50.88    3.601 
52.93     3.667 

BENZENE  AND  WATER  AT  20°, 

(Vaubel  —  J.  pr.  Ch.  [2]  67,  476.  'cj-) 


Volumes  of  Solvents 

used  per 
i  Gm.  Phenol 

5occ.H2O  +  5occ.C6H6 

"  +IOOCC.    " 

+  I50CC.  " 

+  200CC.    " 


Gms.  Phenol  in- 


Layer 


H20 
Layer. 

o.  286  o.  714 
o.  1188  0.8212 
0.0893  0.9107 
0.0893  0.9107 


225 


PHENOL 


DISTRIBUTION    OF    PHENOL    BETWEEN    WATER    AND    BENZENE    AND 
BETWEEN  AQUEOUS  K2SO4  SOLUTIONS  AND  BENZENE  AT  25°. 

(Rothmund  and  Wilsmore  —  Z.  physik.  Ch.  40,  623,  '02.) 

NOTE.  —  The  original  results,  which  are  given  in  terms  of  gram 
mols.  per  liter,  were  calculated  to  grams  per  liter,  and  plotted  on  cross- 
section  paper.  The  following  figures  were  read  from  the  curves 
obtained. 


Between  H2O  and 


Effect  of  K2SO4  upon  the  Distribution. 


Grams  C8H5OH 

Cms.  K2SO4 

(i)  Gms. 

C6H5OH 

(2)Gms.  C6H5OH 

per  Liter  of: 

per  Liter 

per  Liter  of: 

per  Liter  of: 

H20 
Layer. 

C6H6 
Layer. 

Aq. 
Solution. 

Aq. 
Layer. 

C6H8 
Layer. 

Aq. 

Layer. 

C6H8 
Layer. 

5 

10 

I.36 

17.08 

59-96 

9-52 

26.28 

10 

28 

2.72 

16.92 

60-63 

9-5° 

26.38 

15 

52 

5-44 

16.85 

60.92 

9-46 

26-55 

20 

84 

10.89 

16.44 

62.73 

9-35 

27  .06 

25 

128 

21.79 

15.89 

65.19 

9.09 

28.27 

30 

2OO 

43-59 

I4-85 

69.71 

8.68 

30.21 

35 

300 

87.18 

12  .92 

78.00 

7-79 

34.38 

40 

4IO 

45 

520 

50 

610 

(i)  First  series. 

(2) 

Second  series. 

DISTRIBUTION  OF  PHENOL  AT  25°  BETWEEN: 

(Herz  and  Fischer  —  Ber.  38,  1143,  '05.) 


Water  and  Toluene. 

Millimols 

CbH6OH 

Grams  C6H5OII 

per  10  cc. 

per  100 

cc. 

C6H5CH3 

Layer. 

H2O 
Layer. 

C6H5CH3 
Layer. 

H26 
Layer. 

1.244 

0.724 

1.169 

0.681 

3-°47 

1.469 

2.865 

1.381 

4.667 

2  .200 

4-389 

2.068 

6.446 

2.861 

6.o6l 

2  .691 

14.960 

4-75° 

14.07 

4.467 

17.725 

5-346 

16.69 

5.027 

47.003 

7.706 

44-20 

7.246 

53-783 

8.087 

50.58 

7.604 

90.287 

9.651 

84.89 

9.074 

Water  and 

Millimols  C6H5OH 
per  10  cc. 

m  Xylene. 

Grams  C6H6OH 
per  100  cc. 

'  mC6H4(CH3)2        H20  *     ' 
Layer.            Layer. 

1.610       1.071 

4.787         2.726 

12.210       5-i68 
22.718       6.994 
34.827       8.124 
5I-352       9-123 
77.703     10.050 

™C6H4(CH3)2     H20" 
Layer.         Layer. 

1.514       1.007 
4.501       2.563 
11.22          4.860 
21.36         6.577 
32.75          7.640 
48.28         8.578 
73-07          9-450 

DISTRIBUTION    OF    PHENOL    BETWEEN    WATER    AND    CARBON    TETRA 

CHLORIDE  AT  20°. 

(Vaubel  — J.  pr.  Ch.  [2]  67,  476,  '03.) 

Grams  Phenol  in: 


Cms.  Phenol 
Used. 


Volumes  of  Solvents. 

i       50  cc.  H2O+   10  cc.  CC14 

I  "       '      +     20  CC.  " 

+  30  cc.  " 

+  50  cc.  " 

"  +IOOCC.  " 

+  i5occ.  " 

-f200CC.  " 


H20  Layer. 

CC14  Layer. 

0.8605 

0.1285 

0.7990 

o  .  1900 

0.7275 

O.26l5 

0-6435 

0-3455 

o  .  4680 

0.5210 

0.3645 

0.6245 

0.3240 

0-6650 

PHENOLATE  226 

PHENOLATE   of    Phenyl   Ammonium. 

SOLUBILITY  IN  WATER. 

Figures  read  from  Curve.    (Alexejew  —  Wied.  Ann.  28,  305,  '86.) 

By  Synthetic  Method,  See  page  9. 

Gms.  Phenolate  per  100  Gms.  0  Gms.  Phenolate  per  100  Gms. 

Aq.  Layer.     Phenolate  Layer.  Aq.  Layer.     Phenolate  Layer. 

10  3  94  no  9  76 

30  4  93  I2°  I2  69 

50  5  91  130  17.5  60 

70  6  87.5  140  (crit.  temp.)  40 

90  7  83 


PHENYL    (Di)    AMINES    C6H4(NH2)2. 

SOLUBILITY  IN  WATER  AT  20°. 

(Vaubel  — J.  pr.  Ch.  [2]  52,  73,  '95-) 

A     •_  Gms.  per  ioo  Sp.  Gr.  of 

Gms.  Solution.  Solution. 

m  Phenyl  di  Amine  23 .8  1-0317 

P  3-7  1-0038 


Nitro    PHENOLS    C6H4.OH.NO2. 

ioo  grams  saturated  aqueous  solution  contain:  0.208    gram  ortho, 
2.14  grams  meta,  1.32  grams  para  nitro  phenol  at  20°. 

(Vaubel.) 

Di   Nitro    PHENOL   C6H3.OH.(NO2)2. 

SOLUBILITY  IN  ALCOHOLS  AT  19.5°. 

(de  Bruyn  —  Z.  physik.  Ch.  10,  784,  '92.) 

ioo  grams  abs.  methyl  alcohol  dissolve  6.3  grams  C6H3.OH.(NO2)2. 
ioo  grams  abs.  ethyl  alcohol  dissolve  3^9  grams  C6H3.OH.(NO2)2. 

SOLUBILITY  OF  MIXTURES  OF  5  TRI  BROM  PHENOL  AND  5  TRI  CHLOR 
PHENOL  IN  METHYL  ALCOHOL  AT  25°. 

(Thiel  —  Z.  physik.  Ch.  43,  667,  '03;  from  Wurfel  —  Dissertation  Marburg,  '96.) 
Molecular  per  cent  C6H2.OH.Br3  n  Solubility  of 


'  In  Solid. 

In  Solution. 

CeH2.OH.Cl3. 

C6H2.OH.Br3. 

i  oiai. 

0 

O 

O.204 

O 

0.204 

4-49 

3-59 

0-194 

0.007 

0.201 

10.13 

7-58 

O.I9I 

0.016 

O.2O6 

16.28 

12.15 

0.172 

O.O24 

0.196 

62.44 

13.07 

O.2O4 

O.O3I 

0-235 

69.88 

15.86 

0.150 

0.028 

0.178 

81.76 

19.01 

0.096 

0.023 

O.IlS 

84.66 

24.05 

0-069 

O.O22 

O.O9I 

87-53 

32.46 

0.043 

0-021 

0.063 

93.62 

47-87 

O-O2I 

0.019 

O.O4O 

IOO.O 

IOO.O 

0-0 

O.OI9 

O.OI9 

227  PHENYL    SALIC YL ATE 

PHENYL    SALICYLATE    (Salol)  C6H4(OH).COOC6H6i:2. 

100  grams  H2O  dissolve  0.043  STarn-  salicylate  at  25°.     100  grams 
alcohol  dissolve  20.0  grams  at  25°. 

(u.  s.  P.) 


Di    PHENYL   C6H5.C6H6. 

100  grams  absolute  methyl  alcohol  dissolve   6.57   grams  at   19.5°. 
100  grams  abs.  ethyl  alcohol  dissolve  9.98  grams  at  19.5°. 

(de  Bruyn  —  Z.  physik.  Ch.  10,  784,  '92.) 


PHOSPHO    MOLYBDIC    ACID    P2O5.2oMoO3.52H2O. 

SOLUBILITY  IN  ETHER. 

(Parmentier  —  Com pt.  rend.  104,  686,  '87.) 

t°  o°         8.1°  19.3°     27.4°     32- 9C 

Gms.  Acid  per  100  gms.  Ether    80.6    84.7     96.7     103.9     107.9 


PHOSPHORUS    P.  (yellow) 

SOLUBILITY  IN  BENZENE. 

(Christomanos  —  Z.  anorg.  Ch.  45,  136,  '05.) 

.  o  Gms.  P  pel 

•  i oo  Gms.  C61 

50  6.80 

55  7-32 

60  7 . 90 

65  8.40 

70  8.90 

75  9-4o 

81  10.03 


Gms.  P  per 

t  °.       100  Gms. 

(C2H6)20. 

28  1. 60 

30  i-75 
33  i -80 
35  2.00 


100  grams  CS2  dissolve  about  1750  grams  yellow  P  at  room  temper- 
ature. (Vogel  —  Jahresber.  Chem.  149,  '68.) 

ioo  grams  alcohol  of  0.799  Sp.  Gr.  dissolve  0.312  gram  P  cold  and 

0.416  gram  hot.  (Buchner) 


-o         Gms.  P  per 
'     iooGms.C6H6. 

Sp.  Gr.  of] 
Solution. 

-o         Gms.  P  per 
"    100  Gms.  CeHe. 

Sp.  Gr.  of 
Solution. 

O 

1.513 

.  .  . 

23 

3-399 

0-8875 

5 

1.99 

25 

0.8861 

8 

2.31 

o  .  8990 

30 

4.60 

10 

2.4 

0.8985 

35 

5  •I7 

15 

2-7 

0-894 

40 

5-75 

18 

3  -1 

0.892 

45 

6.  ii 

20 

3-2 

0.890 

SOLUBILITY 

OF  PHOSPHORUS 

IN  ETHER. 

(Christomanos.) 

... 

Gms.  P  per 
loo  Gms. 
(C2H6)20. 

Sp.  Gr.  of 
Solutions. 

f. 

Gms.  P   per 

100  Gms. 
(C2H5)20. 

Sp.  Gr.  of 
Solutions. 

0 

0-434 

15 

0.90 

0.723 

5 

O.62 

.  .  . 

18 

I  .01 

0-719 

8 

0-79 

0.732 

20 

I  -04 

0.718 

10 

0.85 

0.729 

23 

I  .12 

0.722 

25 

i-39 

0.728 

PHOSPHORUS  228 

SOLUBILITY  OF  YELLOW  PHOSPHORUS  IN  SEVERAL  SOLVENTS  AT  15°. 

(Stich  —  Pharm.  Ztg.  48,  343.  '03-) 

Solvent.  Gms.    P  per  100  Gms.  Solution. 

Almond  Oil  i  .25 

Oleic  Acid  i  .06 

Paraffine  i .  45 

Water  0.0003 

Acetic  Acid  o .  105 


PHTHALIC    ACIDS    C6H4(COOH)2. 

SOLUBILITY  IN  WATER. 

(Vaubel  — J.  pr.  Ch.  [2]  52,  73,  '95;  59,  30,  '99-) 
Acid.  t  °.  Gms.  per  100  Gms.  Solution. 

o  Phthalic  Acid  14  0.54 

Iso  Phthalic  Acid  25  0.013 

Tere  Phthalic  Acid  . .  almost  insoluble 

SOLUBILITY  OF  o  PHTHALIC  ACID  IN  ALCOHOL  AND  IN  ETHER  AT 

(Bourgoin  —  Ann.  chim.  phys.  [5]  13,  406,  '78.) 

Grams  CeH^COOETte  o  per  TOO  Grams 
Solution.  Solvent. 

Absolute  Alcohol  9 . 1 56  1 1 . 70 

90  per  cent  Alcohol  10.478  10.08 

Ether  0.679  0.684 


TO 
PHTHALIC    ANHYDRIDE    C6H4<co>O- 

SOLUBILITY  IN  WATER. 

(van  der  Stadt  —  Z.  physik.  Ch.  41,  358,  '02.) 

All  determinations,  except  first  three,  made  by  the  Synthetic  Method. 
See  page  9. 


t°. 

irams  CgKjOa  per  100  Gms.  Mol.  i 

>er  cent 

Grams  Cg^Os  per  100  Gms.   M°l. 

^  °0                                                                                       r*»r  «-oTif 

Water. 

Solution.        Q^Os- 

Water. 

Solution. 

C8H403 

0 

O, 

,00295 

0. 

00295 

0 

.  00036 

189.5 

1076 

91. 

66 

56.73 

25 

0. 

6194 

O. 

6150 

o 

•°754 

188.8 

1265 

92. 

68 

60.63 

50 

I, 

630 

I. 

604 

0 

.198 

187.1 

1474 

93- 

65 

64.  22 

135-9 

94. 

•3 

48. 

54 

10 

•30 

181.8 

2332 

95- 

88 

73-95 

165.4 

210, 

o 

67. 

75 

20 

•36 

176.2 

3334 

97- 

07 

80.23 

179.4 

319 

3 

76. 

13 

27 

.98 

169.4 

5745 

98. 

28 

87.49 

186.2 

449. 

6 

81. 

81 

35 

•37 

130.9 

37570 

99- 

72 

97.89 

189.6 

546. 

i 

84. 

5° 

39 

•93 

131.0 

83010 

99- 

86 

99.02 

191.0 

821. 

5 

89. 

19 

5o 

.00 

131.2 

oo 

100. 

00 

100.  OO 

190.4 

863.4                  89. 

62 

.24 

On  page  362  of  the  original  paper  the  solubility  of  C8H4O3  at  o°  is 
given  as  0.2722  gram  per  100  grams  of  solution. 


229  PHTHALIO    ANHYDRIDE 

SOLUBILITY  OF  PHTHALIC  ANHYDRIDE  IN  CARBON  BISULPHIDE. 

(Arctowski  —  Compt.  rend.  121,  123,  '95;  Etard  —  Ann.  chim.  phys.  [7]  2,  570,  '94.) 


Gms.  CgH4O3 

Gms.  C8H4O3 

Gms.  C8H4O3 

f. 

per  loo  Gms. 
Solution. 

t°.  per  100  Gms.             t°. 
Solution. 

per  loo  Gms. 
Solution. 

— 

112.5 

0.013 

+  10 

°-3 

70 

2-3 

— 

93 

0.013 

2O 

0.7 

90 

3-7 

— 

77-5 

0.016 

30 

0.8 

IOO 

5-o 

— 

40 

0.03 

40 

I  .2 

I2O 

8.0 

— 

20 

O.O6 

50 

I  .3 

I4O 

13-3 

— 

10 

o.io 

60 

I  .7 

1  60 

20.7 

0 

O.2O 

180 

30.2 

PHYSOSTIGMINE    SALICYLATE    C6H4(OH)COOH.C16H21N3O2    and 
Physostigmine    Sulphate    H2SO4(C15H21N3O2)2. 


SOLUBILITY  IN  WATER,  ALCOHOL,  ETC. 

(U.  S.  P.) 

Gms.  per  100  Gms.  Solvent. 

Solvent.  t°.  -— — -i- • » 

bahcylate.  Sulphate. 

Water  25  1.38       very  soluble 

Water  80  6.66 

Alcohol  25  7.87 

Alcohol  60  25.00 

Chloroform  25  n.6  " 

Ether  25  °-57          0.083 


PICRIC    ACID    C6H2.OH.(NO2)3. 

SOLUBILITY  IN  WATER. 

(Dolinski  —  Ber.  38,  1836,  '05;  Findlay  —  J.  Ch.  Soc.  81,  1219,  '02.) 
Gms.  CeHaNgOy  per  100  Grams  Gms.  CeHaNsOr  per  100  Grams 


Solution.                               Water.  Solution.                            Water. 

o  0.67  (D.)  0.68  (D.)  1.05  (F.)  60  2.77(0.)   2.81(0.)  3-i7 

10  .80  0.81    1. 10  70  3.35  3.47  3-89 

2O  I. 10  I. II     1-22  80  4-22  4.41  4.66 

30  1.38  1.40    1.55  90  5.44  5-72  5-49 

40  1.75  1.78    1.98  loo  6.75  7.24  6.33 

50  2.15  2.19   2.53 


Dolinski  does  not  refer  to  the  previous  determinations  of  Findlay 


PICKIO  ACID 


230 


SOLUBILITY  OF  PICRIC  ACID  IN  WATER  AND  IN  AQUEOUS  SALT 
SOLUTIONS  AT  25°. 

(Levin  —  Z.  physik.  Ch.  55,  520,  '06.) 

One  liter  of  aqueous  solution  contains  0.05328  gram  mols.  =  12.20 
grams  C6H2.OH(NO2)3  at  25°. 

Gm  Mols  Salt  Gram  Mols.  Picric  Acid  per  Liter  in  Aq.  Solutions  of: 


per  Liter. 

NaCl. 

NaNO3. 

Na2S04. 

LiCl. 

Li2S04. 

NH4C1. 

0 

.01 

0 

•05524 

0.05529 

0-05604 

0.05480 

O 

.05661 

0.05487 

0 

.02 

0 

•05559 

0-05872 

0-05872 

0-05558 

0 

.06053 

0.05540 

O 

•05 

0 

.05729 

0.06632 

o  .06632 

0.05703 

0 

.06691 

0.05771 

0 

.07 

0 

.05862 

0.07093 

0.07093 

0.05878 

o 

•07013 

0.05865 

0 

.10 

0 

.05902 

0.07670 

0.07670 

0.06132 

o 

•07437 

O 

•50 

0 

.0790 

0 

.123 

I 

.00 

0 

.Il8o 

0 

.149 

Gm. 

Mols. 

Grams  Picric  Acid  per 

Liter  in  Aq.  Solutions  of: 

Salt  per  Liter. 

NaCl. 

NaN03. 

Na2S04, 

LiCl. 

Li2S04. 

NH4C1. 

O 

.01 

12  .66 

12.67 

12.83 

I2-55 

12.97 

12-57 

O 

•  O2 

12.74 

13-45 

*3-45 

12-74 

13-87 

12  .69 

O 

•05 

13.12 

I5-J9 

15  -19 

13.06 

15-33 

13.22 

0 

.07 

13-43 

16.25 

16.25 

13-47 

16.06 

13-44 

O 

.10 

J3-52 

17-57 

17-57 

14.05 

17.04 

O 

•50 

18.09 

28.18 

I 

.00 

26.98 

34-14 

Solubility  in  Aq.  Cane  Sugar. 


Solubility  in  Aq.  Grape  Sugar. 


Jm.  Mols. 
Sugar 
per  Liter. 

Picric  Ac.  per  L 

iter  Solution. 

Sp.  Gr. 
Solution. 

Gm.  Mols. 
Grape  Sugar 
per  Liter. 

Picric  Acid  rxr  Liter  Sol. 

Gm.  Mols. 

Gms. 

G.  Mols. 

Gms. 

O.IO 

O.O52O2 

II  .92 

I  -OI22 

O.IO 

0.0530 

12  .14 

0.25 

0.04978 

II    40 

1.0319 

0.25 

0.0521 

11  -93 

0.50 

0.0482 

II  .04 

I  .0654 

0.50 

0.0509 

11.66 

I  .00 

0.0443 

IO.I5 

I.I294 

I  .00 

0-0474 

10.86 

SOLUBILITY  OF  PICRIC  ACID  IN  ABSOLUTE  ALCOHOL. 

(Behrend  —  Z.  physik.  Ch.  10,  265,  '92.) 


ioo  gms.  sat.  solution  contain  5.53    grams  CgHg 
5.92  grams  at  14.8°.     Sp.  Gr.  of  the  latter  solution 


y  at  12.3°,   and 
0.8255. 


5 
10 

20 

25 
?6.5 

35 


SOLUBILITY  OF  PICRIC  ACID  IN  BENZENE. 

(Findlay.) 


Gms. 

Mols. 

Gms. 

Mols. 

C6H3N307 

C6H3N307 

t°. 

C6H3N307 

per  ioo 

per  ioo 

per  ioo 

per  ioo 

Gms.  C6H6. 

Mols.  C6H6. 

Gms.  C6H6. 

Mols.C6H 

3-70 

1.26 

38.4 

26.15 

8.88 

5-37 

I-83 

45 

33-57 

II  .40 

7.29 

2.48 

55 

50-65 

17  .21 

9.56 

3-25 

58-7 

58.42 

19.83 

12.66 

4-3° 

65 

71  .31 

24.2O 

13  .51 

4.60 

75 

96.77 

32.92 

21.38 

7.26 

23I 


PICRIC    ACID 


SOLUBILITY  OP  PICRIC  ACID  IN  ETHER. 

(Bougault  —  J.  pharm.  chim.  [6]  18,  116,  '03;  — Apoth.-Ztg.  21,  74,  '06.) 


Solvent.  t°. 

Ether  of  Sp.  Gr.  0.721  13 

Ether  of  Sp.  Gr.  0.725  (0.8  pt.  H2O  per  100)  13 

Ether  of  Sp.  Gr.  0.726  (i.o  pt.  H2O  per  100)  i^ 

Ether  saturated  with  H2O  15 

H2O  saturated  with  Ether  15 


Cms.  C«H3N3O7  per  Liter. 

10.8         (B.) 

36.8 
40.0 

5*-2 

13-8 


DISTRIBUTION  OF  PICRIC  ACID  AT  25°  BETWEEN: 


Water  and  Amyl  Alcohol. 

(Herz  and  Fischer  —  Ber.  37,  4747,  '04.) 


Water  and  Toluene, 

(H.  and  F.  — Ber.  38,  1142,  '05.) 


Millimols  CsHsNsCv 

Cms.  C6H3N3O7 

Millimols 

C6H3N,07 

Cms. 

C6H3N307 

per 

10  CC. 

per  loo  cc. 

per 

10  CC. 

per 

100  CC. 

Aq. 

Alcohol 

Aq. 

Alcohol 

Aq. 

Toluene 

Aq. 

Toluene 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

0-0553 

o  .  0930 

O.I27 

0-2I3 

0.075 

O.I26 

0.172 

0.289 

O.092O 

0.1850 

O.2II 

0.424 

O.IO9 

0.230 

o  250 

0.527 

O.l6l3 

0.4127 

0-369 

0.946 

0.163 

0.482 

o-374 

I  .104 

0.1869 

0.5182 

0.428 

1.188 

0.244 

I  .026 

o-559 

2-351 

0.3161 

1.079 

0.724 

2-473 

0.389 

2-347 

0.891 

5-38o 

0.4471 

1.638 

I  .024 

3-753 

0.496 

3-747 

1  .137 

8.586 

0.5624 

2.189 

1.288 

5-oi7 

0-583 

5-I35 

1  .336 

11.770 

0.6423 

2-549 

1.472 

5-839 

DISTRIBUTION  OF  PICRIC  ACID  AT  25°  BETWEEN: 


Water  and  Bromoform. 

(Herz  and  Lewy  —  Z.  Electrochem.  u,  820,  '05.) 


Water  and  Chloroform. 

(H.  and  L.) 


Millimols  CeHsN3O7 
per  10  cc. 

Cms.  C6H8N307 
per  100  cc. 

Millimols  CeH3N307 
per  10  cc. 

Gms.  Cgri3N3O7 
per  loo  cc. 

Aq.       Bromoform 
Layer.         Layer. 

0.321       0.365 
O.4OI       0.515 

o-475     0.655 
o-575    0.871 
0.674     1.14 

Aq.      Bromoform 
Layer.        Layer. 

0.736      0.836 
0.919       I.lSo 
I.  088       I.50I 

i-3i7     1-995 
1.545     2.612 

Aq.         Chloroform 
Layer.        Layer. 

0.2O7      0.254 

0-329      0-547 
0.488       1.09 
0.561       1.41 
0.588       1.53 

Aq  .         Chloroform 
Layer.          Layer. 

0-474      0.582 

0-754     1-253 
1.118     2.498 
1.285     3.230 
I-348    3.505 

PILOCARPINE    HYDROCHLORIDE      CnH16N2O2.HCl,    Pilocarpine     Ni- 
trate CUH16NA.HNO3,  and  Piperine  C17H19NO3  in  Several  Solvents. 


Solvent. 

Water 

Alcohol 

Alcohol 

Chloroform 

Ether 


25 
2$ 
60 

25 
25 


(U.  S.  P.) 

Grams  per  100  Grams  Solvent. 
Ci,H16N202.HCl.    CiiH16N202.HN03.    C,7H19NO3. 

333  25  insoluble 

4.35  1.66  6.66 

9.09  6.2  22.7 

0.18  ...  58.8 

2.8 


PLATINUM    ALLOYS  232 

•  SOLUBILITY  OF  PLATINUM  ALLOYS  IN  NITRIC  ACID. 

(Winkler  — Z.  anal.  Ch.  13,  369,  '74.) 


Approx.           Grams  Alloy  Dissolved  per  100  Grams  HNOs  Solution  oi 

Alloy  *                      per  cent       /—                                                    ~" 
Pt  in  Alloy. 

i-398Sp.Gr. 

i.298Sp.Gr. 

x.igoSp-Gr. 

i.2g8Sp.Gr.: 

Pt  and  Silver 

10 

57 

44 

69 

37 

" 

5 

69 

57 

51 

35 

tt 

2-5 

62 

61 

69 

11 

i 

75 

70 

76 

Pt  and  Copper 

IO 

46 

27 

II 

51 

" 

5 

36 

34 

14 

" 

2-5 

51 

40 

30 

" 

i 

52 

41 

37 

Pt  and  Lead 

10 

7 

9 

8 

.  . 

" 

5 

8 

9 

10 

" 

2-5 

22 

i7 

ii 

" 

21 

18 

23 

.  . 

Pt  and  Bismuth 

10 

14 

19 

4 

3 

tt 

5 

21 

20 

6 

18 

ti 

2-5 

25 

42 

8 

.  . 

11 

i 

49 

64 

10 

.  . 

Pt  and  Zinc 

10 

10 

II 

19 

5 

" 

5 

16 

12 

6 

ii 

« 

2-5 

16 

24 

19 

.  . 

tt 

i 

20 

32 

37 

PLATINUM    BROMIDE    PtBr4. 

100  grams  sat.  aqueous  solution  contain  0.41  gram  PtBr4  at  20° 

(Halberstadt  —  Ber.  17,  2962,  '84.) 

PLATINIC    POTASSIUM    BROMIDE    K2PtBr6. 

100  grams  sat.  aqueous  solution  contain  2.02  grams  K2PtBr6  at  20°. 

(Halberstadt.) 

PLATINIC    DOUBLE    CHLORIDES  of  Ammonium,  Caesium,  Potas- 
sium,   Rubidium   and   Thallium. 

SOLUBILITY  IN  WATER. 

(Crookes  —  Chem.  News  9,  37,  205,  '64;  Bunsen  —  Pogg.  Ann.  113,  337,  *6i.) 
Grams  per  100  Grams  Water. 


i/  . 

o 

10 

(NH^PtCle.           Cs2PtCl6. 
O.O24 

0.666  (15°)     0.050 

K2PtClfi. 
0-74 
0.90 

Rb2PtCl«. 
0.184 
0.154 

Tl2PtCl6. 
0.0064  (15°) 

20 
25 

0.079 
0.095 

I  .12 
I  .26 

O.I4I 
0.143 

.  .  . 

30 
40 

O.IIO 

0.142 

I.4I 
I.76 

0.145 

0.166 

.  .  . 

So 
60 

0.177 
0.213 

2.17 
2.64 

0.203 
0-253 

. 

7o 
80 

0.251 
0.291 

3-79 

0.329 
0.417 

::: 

90 

100 

0.332 
1.25           0.377 

4-45 

0.521 
0-634 

0.050 

233  PLATINIO      CHLORIDES 

SOLUBILITY  OF  AMMONIUM   PLATINIC  CHLORIDE  AND  OF  POTASSIUM 
PLATINIC  CHLORIDE   IN  ALCOHOL  AT  i5°-2o°. 

(Fresenius;  Peligot  —  Z.  aaal.  Ch.  36,  322,  '97.) 

o,       L         Gms.  per  Liter  Solution.  Cms,  per  Liter  Solution.     ' 

(NH4)2PtCl6.    K2PtCl6.  ' 


55%  Alcohol     0.150        ...       95%  Alcohol  0.0037  0.030 

76                      0.067      0.026    Abs.       "  ...  0.0082-0.002? 
85                         ...         0.180    80  Vol.%  Alcohol  +  20 

Vol.  %  Ether  ...  0.027 

90                                     o.  loo    Abs.  Methyl  Alcohol  .  .  .  0.072 


PLATING    AMINES. 

SOLUBILITY  IN  WATER. 

(Cleve.) 

Amine.  Formula. 

/ATTT  \    pi  Gms.  per  TOO  Gms.  H2O. 

Platino  Semi  Di  Amine  Chloride       Pt  < gj "«>»•  0.26  at  o°  '3.4    at  100° 

Chloro  Platin  Amine  Chloride    *          C12Pt<NHCl      °'14     "        3'°       " 
Chloro  Platin  Semi  Diamine  Chloride  Cl3Pt(NH3)2Cl    o.  33     "        i .  54     " 


POTASSIUM    ACETATE    CH3COOK. 

SOLUBILITY  IN  WATER. 

100  gms.  sat.  aq.  solution  contain  73.65  gms.  CH3COOK,  or  100 
gms.  H2O  dissolve  286.3  gms.  at  31.25°. 

(Kohler  —  Z.  Ver.  Zuckerind.  47,  447,  '97.) 

ioo  gms.  H2O  dissolve  188  gms.  CH3COOK  at  5°,  229  gms.  at  13.9°, 
492  gms.  at  62°. 

(Osann.) 

ioo  gms.  99  per  cent  ethyl  alcohol  dissolve  33.3  gms.  CH3COOK  at 
15°,  and  50.0  gms.  at  80°. 


POTASSIUM    (Di   Hydrogen)    ABSENATE    KH2AsO4. 

ioo  gms.  sat.  aq.  solution  contain  15.9  gms.  KH2AsO4,  or  ioo  gms. 
H,O  dissolve  18.86  gms.  at  6°.     Sp.  Gr.  of  solution  =  1.1134. 

(Field  — J.  Ch.  Soc.  n,  6,  '59.) 


POTASSIUM    BENZOATE    KC7H5O2.3H2O. 

SOLUBILITY  IN  WATER. 

(Paietta  —  Gazz.  chim.  ital.  36,  II,  67,  '06.) 
t°-  17-5°  25°  33.3°  50° 

Gms.  KC7H5O2  per  ioo  Gms.    41.4  42.4          44.0         46.6 

Solution. 


POTASSIUM    BORATES 


234 


SOLUBILITY  OF  POTASSIUM  BORATES  IN  WATER  AT  30°. 

(Dukelski  —  Z.  anorg.  Chem.  50,  42,  '06,  complete  references  given.) 


Gms.  per  100  Gms.  Solution.      Gms.  per  100  Gms.  Residue. 


K20. 

B203. 

K20. 

B203. 

47-50 

46.36 

0.91 

46.13 

9-O2 

40.51 

1-25 

41  .62 

9.71 

36.82 

1.  80 

39-90 

32-74 

3-51 

37-22 

14.58 

29.63 

6.98 

35-05 

17.92 

24-84 

17.63 

30.02 

21  .70 

23-30 

18.19 

26.84 

31-49 

16.21 

13.10 

25  >I2 

33-18 

11.78 

9.82 

20-57 

26.43 

9.18 

8.00 

22.38 

3I-30 

6.22 

9.13 

20.87 

31.06 

7-73 

13-37 

22.21 

36.24 

7.8! 

13.28 

I7-50 

34.18 

7.71 

13.21 

11-49 

34-81 

7-63 

13.28 

I2-5I 

40.52 

3  42 

7-59 

10-77 

37-35 

i.  80 

4-i5 

5.88 

20  oo 

0.51 

3-J9 

I0.8l 

40.89 

o-33 

4.58 

7-72 

34-21 

0.31 

4.46 

3-91 

30.68 

3-54 


Solid 
Phase. 

KOH.2H2O 
K2O.B203.2iH2O 


K2O.2B2O3.4H2O  +K2O.sB203.8H2O 
K2O.5B203.8H2O 


K2O.sB2O3.8H2O+  B(OH)3 


POTASSIUM    (Fluo)    BORIDE    KBF4. 

100  gms.  H2O  dissolve  0.44  gm.  KBF4  at  20°,  and  6.27  gms.  at  100° 

(Stolba  —  Chem.  techn.  Centr.  Anz.  7,  459,  '89.) 


POTASSIUM    BROMATE    KBrO,. 


SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg.  Ann.  97,  5,  '56;  Rammelsberg  —  Ibid.  55,  79,  '42;  Pohl  —  Sitzber.  Akad.  Wiss 
Wien.  6,  595,  '51.) 


Gms.  KBrO3  per  100  Gms. 


Gms.  KBrO3  per  100  Gms. 


ll    . 

Water. 

Solution. 

t  . 

Water. 

Solution. 

0 

3    ! 

3-o 

40 

I3.2 

ii.  7 

10 

4.8 

4.6 

50 

17-5 

14.9 

20 

6.9 

6-5 

60 

22  .7 

18.5 

25 

8.0 

7-4 

80 

34  o 

25  4 

30 

95 

8.7 

100 

50-0 

33-3 

Sp.  Gr.  of  solution  saturated  at  19.5°  =  1.05. 


235  POTASSIUM    BROMATE 

SOLUBILITY  OF  POTASSIUM  BROMATE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  NITRATE  AND  OF  SODIUM  CHLORIDE. 

(Geffcken  —  Z.  physik.  Chem.  49,  296,  '04.) 

In  Sodium  Nitrate.  In  Sodium  Chloride. 

Grams  per  Liter.  Mols.  KBrO3  Grams  per  Liter.  Mols.  KBrO3 

NaNO3.          KBrO3.  Per  Liter-  NaCl.  KBrO3.  Per  Liter. 

o.o    78-79  0.4715  °-°    78  79  0.4715 

42.54   96.01  0.5745  29  25    82.24  0.5220 

85.09  108.6  0.6497  58-5o    93 .87  0.5616 

170.18  128.3  0.7680  117.0  100.9  0.6042 

255.27  150-9  0.9026  I75-5  IO4  3  0.6244 

340.36  1/2.3  1-031  234.0  106.9  0.6400 

POTASSIUM    BROMIDE    KBr. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Meusser  —  Z.  anorg.  Chem.  44,  79,  '05;  Etard  —  Compt.  rend.  98,  1432, 

'84;  Ann.  chim.  phys.  [?J  2,  526,  '94;  de  Coppet  —  Ibid.  [5]  30,  416,  '83;  Tilden  and 

Shenstone  —  Phil.  Trans.  175,  23,  '84.) 

Grams  KBr  per  100  Grams  Grams  KBr  per  100  Grams 


Solution. 

Water. 

Solution. 

Water. 

— 

6 

•5 

20. 

0 

25.0 

30 

41.4 

70.6 

— 

8, 

c 

26. 

5 

35 

•7 

40 

43-o 

75-5 

— 

10 

5 

29. 

e 

41 

.8 

50 

44-5 

80.2 

— 

n 

31 

2 

45-3 

60 

46.1 

85-5 

— 

IO 

31- 

8 

46 

•7 

70 

47-4 

90.0 

— 

5 

33- 

3 

5o 

.0 

80 

48.7 

95-o 

o 

34- 

9 

53 

•5 

90 

49-8 

99-2 

5 

36- 

i 

56 

•5 

IOO 

51.0 

104.0 

10 

37- 

3 

59 

•5 

no 

52-3 

109  .  5 

15 

38- 

5 

62 

•5 

140 

54-7 

120.9 

20 

39- 

5 

65 

.2 

181 

59-3 

145.6 

25 

40. 

4 

67 

•7 

SOLUBILITY  OF 

MIXTURES  OF  POTASSIUM  BROMIDE  AND 

AMMONIUM 

BROMIDE  IN 

WATER  AT  25 

0 

(Fock  — 

Z.  Kryst.  Min. 

28,  357.  '97-) 

Grams  per  Liter  Solution. 

Mol.  per  cent  in  Solution. 

Sp.  Gr.  of 

Mol.  per  cent 

in  Solid  Phase 

NH4 

Br. 

KBr 

NH4Br. 

KBr. 

Solutions. 

NH4Br. 

KBr. 

o. 

OO 

558- 

i 

o.o 

IOO 

I-3756 

0 

.00 

IOO 

6. 

4 

554- 

2 

1.38 

98. 

62 

1-3745 

O 

.26 

99-74 

24. 

64 

536. 

5 

5-29 

94- 

71 

1-3733 

I 

.27 

98.73 

SI' 

34 

516- 

8 

10-77 

89. 

23 

1.3721 

2 

.02 

96.98 

152  . 

9 

441. 

2 

29.63 

70- 

37 

i  .3711 

8 

.42 

9I-58 

262  . 

2 

347- 

3 

47.84 

52- 

16 

*  -37*5 

17 

.20 

82.80 

347- 

6 

262  . 

3 

61  .69 

38. 

31 

1-3753 

27 

.98 

72.02 

4 

260. 

3 

64.03 

35- 

97 

1-3753 

32 

53 

67.47 

417  . 

8 

232. 

2 

68.  61 

31- 

39 

1.3766 

39 

45 

60-55 

432- 

5 

222.3 

70.27 

29. 

73 

1-3777 

variable 

variable 

480. 

8 

179. 

9 

76.47 

23- 

53 

1.3766 

98 

•53 

i-47 

577- 

3 

o. 

o 

IOO.O 

o. 

o 

1-3763 

IOO 

.0 

o.oo 

POTASSIUM    BROMIDE 


236 


SOLUBILITY  OF  POTASSIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OP 
POTASSIUM  HYDROXIDE. 

(Ditte  —  Compt.  rend.  124,  30,  '97.) 


Grams  per  1000  Grams  H2O. 
KOH.  KBr.      ' 

36.4  558.4 

IJ3-5  433-6 

177.2  358.1 

231.1  281.2 


Grams  per  1000  Grams  HgO. 
KBr. 
248.1 


KOH. 
277.6 

434-7 
579.6 
806.9 


64.8 
33.4 


VOLUBILITY  OP  MIXTURES  OF  POTASSIUM  BROMIDE  AND  CHLORIDE  AND 
OF  MIXTURES  OF  POTASSIUM  BROMIDE  AND  IODIDE  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  3,  275,  '97.) 

Mixtures  of  KBr  and  KC1.          Mixtures  of  KBr  and  KI. 

0  Grams  per  TOO  Gms.  Solution.        Grams  per  100  Grams  Solution. 


v  •    * 

KBr. 

KCL 

—  20 

17-5 

10.5 

O 

21-5 

10.8 

10 

23.2 

II  .0 

20 

24.8 

II  .2 

25 

25-5 

"•3 

30 

26.3 

11.4 

40 

28.0 

"•5 

60 

30.6 

ii.  8 

80 

33-4 

12  .1 

100 

35-7 

12.6 

1  20 

38.0 

12-9 

150 

40.6 

I3'4 

KBr. 
9.2 

Kl. 
42-5 

9.9 
IO.2 

45-3 
46.6 

10.5 
10-7 
10-9 
II  .2 

47-5 
48.0 
48.6 
49.6 

ii.  9 

12.6 

5*-3 
52-7 

13.2 

53-8 

14.0 

54-8 

14.9 

55-5 

SOLUBILITY  OP  POTASSIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  CHLORIDE,  AND  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS 
SOLUTIONS  OF  POTASSIUM  BROMIDE,  AT  25.2°. 

(Touren  —  Compt.  rend.  130,  1252,  'oo.) 


KBr  in  Aq.  KCl  Solutions. 

Mols.  per  Liter.                  Grams  per  Liter. 

KCl  in  Aq. 

Mols.  per  Liter. 

KBr  Solutions. 

Grams  per  Liter. 

KCl. 

KBr. 

KCl. 

KBr. 

KBr. 

KCl. 

KBr. 

KCl. 

0.0 

4 

,76l 

O-O 

567 

.0 

0 

.0 

4.18 

0 

.00 

3II.8 

0.67 

4 

.22 

50.0 

502 

•5 

O 

•49 

3.85 

58 

•4 

287.2 

0.81 

4 

.15 

60.4 

494 

.2 

0 

•85 

3-58 

101 

•3 

267.1 

I  .35 

0 

.70 

100.7 

440 

•7 

I 

•31 

3-19 

156 

.1 

238.0 

1.48 

3 

•54 

110.4 

421 

.6 

I 

.78 

2  .91 

211 

•9 

217  .1 

1.61 

o 

,42 

I2O.O 

407 

.2 

2 

•25 

2.58 

268 

.0 

192.4 

1.70 

o 

34 

126.8 

397 

•7 

2 

.69 

2-33 

320 

•4 

173-8 

2.46 

2 

•50 

183.5 

297 

•7 

3-775 

0 

•525 

28J.6 

625 

•3 

237 


POTASSIUM    BROMIDE 


SOLUBILITY  OF  POTASSIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  NITRATE,  AND  OF  POTASSIUM  NITRATE  IN  AQUEOUS 
SOLUTIONS  OF  POTASSIUM  BROMIDE,  AT  14.5°  AND  AT  25.2°. 

(Touren  —  Compt.  rend.  ^30,  908,  'oo.) 

KBr  in  Aqueous  KNO3  Solutions.          KNO3  in  Aq.  KBr  Solutions. 

Mols.  per  Liter.  Grams  per  Liter.  Mols.  per  Liter.  Grams  per  Liter. 


KN03. 

KBr. 

KN03. 

KBr. 

KBr. 

KN03. 

KBr. 

KN03. 

Results  at 

14-2°. 

Results  at  14.20°. 

O-O 

4 

•332 

0 

.0 

5I5-9 

0 

.0 

2.228 

O 

•  O 

225.4 

0-362 

4 

.156 

36 

.6 

494-9 

0 

-356 

2  .026 

42 

•4 

205  .0 

0.706 

4 

•093 

71 

•4 

487.4 

0 

.784 

I-835 

93 

•4 

185-7 

1-235 

3 

•939 

124.9 

469.1 

I 

.092 

1.730 

130 

-0 

J75-o 

I 

•577 

I-587 

I87 

.8 

160.6 

Results  at 

25-2°. 

2 

•542 

I  .406 

302 

•7 

142.2 

0-0 

4 

.761 

O 

.0 

566.2 

3 

•536 

1.308 

421 

.1 

132-3 

O.I3I 

4 

•72 

13 

•3 

561  .0 

Results  at  25.2°. 

0-527 

4 

.61 

53 

•3 

549-1 

0 

•  O 

3.217 

0 

.0 

325-5 

0.721 

4 

•54 

72 

•9 

540.8 

0 

•38 

3.026 

45-3 

306.2 

1.09 

4 

•475 

no 

•3 

533-o 

0 

•93 

2.689 

no 

.8 

272.0 

I  .170 

4 

•44 

118 

•4 

528.8 

I 

•37 

2.492 

163 

.  i 

252  .2 

1.504 

4 

•375 

J52 

.2 

521.1 

I 

.208 

2  -2l6 

J43 

.8 

224.3 

2 

.87 

1.958 

34i 

.8 

198.1 

3 

•55 

1.807 

422 

.8 

182.8 

SOLUBILITY  OF  POTASSIUM  BROMIDE  IN  ALCOHOLS  AT  25°. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  783,  '92;  Rohland  —  Z.  anorg.  Chem.  18,  327,  '98.) 
Grams  KBr  Dissolved  by  100  Gms.  Alcohol  at: 


Alcohol. 


Methyl  Alcohol 
Ethyl  Alcohol 
Propyl  Alcohol 


Room  Temp.  (R.). 
I  .92 

0.28  (Sp.  Gr.  0.81) 
0-055 


25°  (de  B.). 

1.51  Abs.  Alcohol 


SOLUBILITY  OF  POTASSIUM  BROMIDE  IN  AQUEOUS  ALCOHOL. 

(Taylor —  J.  Physic.  Ch.  I,  724,  '96-'97-) 


Results 

at  30°. 

Results 

at  40°. 

Wt.  per  cent  Alcohol 

Gms.  KBr  per  100  Gms. 

Gms.  KBr  per 

100  Gms. 

in  Solution. 

'Sat.  Solution. 

Solvent. 

Sat.  Solution. 

Solvent. 

O 

41  .62 

71.30 

43-40 

76.65 

5 

38.98 

67.25 

40-85 

72.70 

10 

36'33 

63.40 

38-37 

69.00 

20 

31.09 

56-40 

33-27 

62.30 

30 

25.98 

50-I5 

28.32 

56-45 

40 

21  .24 

44-95 

23  .22 

50.46 

50 

16.27 

38-85 

l8.II 

44-25 

60 

II  .50 

32-50 

13  -O2 

37-40 

70 

6.90 

24.70 

7.98 

28.90 

80 

3-°9 

15-95 

3-65 

18.95 

90 

0.87 

8.80 

1.03 

10.45 

100  gm.  acetone  dissolve  0.023  gm.  KBr  at  25* 

(Krug  and  McElroy 


J.  anal.  Chem.  6,  184,  '92.) 


POTASSIUM    BROMIDE 


238 


Aqueous  Acetone. 


cc.  Acetone 


I0°  cc-  Sat.  Solution. 


per  ioo  cc. 

Millimols 

Gms. 

Gms. 

Solvent. 

KBr. 

KBr. 

H20. 

O 

481.3 

57-3 

80.6 

2O 

366.7 

43-67 

69-5 

30 

3*0-5 

36.98 

62.97 

40 

259.0 

30.85 

55-60 

50 

2O2  .9 

24.16 

47-60 

60 

144.9 

17  .22 

39-15 

70 

95-3 

n-35 

29.78 

80 

46-5 

5-54 

2O.  IO 

90 

IO.I 

I  .20 

IO.I5 

PASSIUM 
—  Z.  anorg. 

BROMIDE  AT  25°  IN: 

Chem.  45,  262,  '05.) 

Aqueous  Glycerine. 

Wt 

.  %      KBr  per  100  cc 

.Sol. 

Sp.  Gr. 
Solutions. 

Glyc 
in  Sc 

Srine 
vent. 

Millimols. 

Gms. 

1-3793 

0 

481 

•3 

57 

•32 

1.2688 

13 

.28 

444 

•3 

S2 

.91 

i.  2118 

25 

.98 

404 

.0 

48 

•  IT 

i  .1558 

45 

•36 

340 

•5 

40 

•55 

i  .0918 

54 

•23 

310 

•4 

36 

.98 

1.0275 

83 

.84 

219 

•25 

26 

.11 

0.9591 

100 

•  OO 

172 

•65 

20 

•56 

0.8942 

0.8340 

Sp.  Gr. 
Solutions 

1-3793 
1-3704 


1-3594 


1.3603 
1.3691 


100  cc.  sat.  solution  of  potassium  bromide  in  furfurol  (C4H3O.COH) 

Contain  0.139  gm.   KBr  at  25°.  (Walden  — Z.  physik.  Chem.  55,  713,  '06.) 

POTASSIUM    BUTYRATE    C3H7COOK. 

100  grams  water  dissolve  296.8  grams  C3H7COOK,  or  100  grams 
sat.  solution  contain  74.8  grams  at  31.25°. 

100  grams  of  an  aq.  solution  saturated  with  sugar  and  C3H7COOK 
contain  49.19  grams  sugar  +  34.78  grams  C3H7COOK  +  16.03  grams 

H2O  at  31.25°.  (Kohler  —  Z.  Ver.  Zuckerind.  47,  447,  '97.) 

POTASSIUM    CARBONATE    K2CO3. 


POTASSIUM    (Bi)    CARBONATE    KHCO3. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Mulder;  Dibbits  —  J.  pr.  Chem.  [2]  10,  439,  '74.) 


Grams  K2CO3  per  100  Grams 


1     . 

0 

Solution. 

47-2 

Water. 
89.4 

IO 

20 

52  -2 
52.8 

IO9.O 
112  .O 

30 

53-3 

II4.O 

40 
60 

IOO 

54-o 
56.0 
60.9 

II7.0 
127.0 
156.0 

Grams  KHCO3  per  ioo  Grams 
Solution.  Water. 


21-7 
24.9 
28.1 
31.2 

37-5 


22-4 

27-7 

33-2 
39-o 

45-3 
60.0 


Kohler  (loc.  cit.)  gives  for  the  solubility  of  K2CO3  in  water,  48.91 
grams  K2CO3  per  100  grams  solution,  or  95.9  grams  per  100  grams 
H2O  at  31.25°.  In  saturated  sugar  solution  at  the  same  temperature 
he  finds  56.0  grams  sugar  +  22.24  grams  K2CO3  +  21.76  grams  H2O 
per  loo  grams  sat.  solution.  Engel  (Ann.  chim.  phys.  [6]  13,  366,  '88) 
finds  1 1  i.o  grams  K2CO3  per  100  grams  H2O  or  52.6  grams  per  100  grams 
sat.  solution  at  o°.  Sp.  Gr.  of  solution  =  1.542.  For  potassium  bi  car- 
bonate he  finds  23  grams  KHCO3  per  100  grams  H2O,  or  18.7  grams 
per  loo  grams  solution.  Sp.  Gr.  of  solution  =  1.127. 


239      POTASSIUM    CARBONATE 

SOLUBILITY  OF  POTASSIUM  Bi  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  CARBONATE  AT  o°. 

(Engel.) 

Milligram  Mols.  rjer  10  cc.  Solution.        £p.  Gr.  of  Grams  per  100  cc.  Solution. 

'  *K2C03. KHC03  Solutions.  '  K2CO3.  KHCO3." 

o.o  21.15  I-I33  o.o  21.2 

17.14  15-28  1.182  ii. 8  15.3 

24.10  12.65  I-2°3  16.7  12.6 

34.50         10.25         1.241         23.8         10.3 

49-20  7.55  1.298  34.0  7.6 

62.14  5.86  i-35°  43-°  5-9 

74.60  4.90  i-398  51-6  4-9 

87.50  3.75  1.448  60.5  3.8 

117.75  °-°  I-542  81.4  o.o 

SOLUBILITY   OF   POTASSIUM   CARBONATE   IN   AQUEOUS   SOLUTIONS   OF 
ETHYL  AND  PROPYL  ALCOHOLS  AT  20°. 

(Linebarger  —  Am.  Ch.  J.  14,  380,  '92;  de   Bruyn  —  Rec.  trav.  chim.  18,  87,  '99.) 

In  Aq.  Ethyl  Alcohol.  In  Aq.  Propyl  Alcohol. 


Wt.  per  cent 
C2H5OH  in 
Solvent. 

Gms.  K2CO3 
per  100  Gms. 
Sat.  Solution. 

Wt.  per  cent 
C2H5OH  in 
Solvent. 

Gms.  K2CO3 
per  100  Gms. 
Sat.  Solution. 

Wt.  per  cent 
C3H7OH  in 
Solvent. 

Gms.  K2CO3  per 
100  Gms. 
Sat.  Solution. 

10 

24 

50 

2-5 

40 

4-3 

20 

16 

55 

1.8 

45 

3-o 

30 

10 

60 

i  .1 

50 

2  -O 

40 

5-6 

65 

0.8 

55 

i-3 

45 

4 

69 

0.4 

60 

0.8 

65 

o-5 

TOO  grams  glycerine  of  1.225  Sp.  Gr.  dissolve  7.4  grams  K2CO3. 

(Vogel  —  N.  Rep.  Pharm.  16,  557,  '67.) 

POTASSIUM    SODIUM    CARBONATE    KNaCO3.6H2O. 

100  gms.  H2O  dissolve  184  gms.  salt  at  15°.     Sp.  Gr.  of  sol.  =  1366. 

(Stolba  —  J.  pr.  Chem.  94,  406,  '65.) 

POTASSIUM    URANYL    CARBONATE    2K2CO3.(UO2)CO3. 
100  gms.  H2O  dissolve  7.4  gms.  salt  at  15°. 

(Ebelmen  —  Liebig's  Ann.  [3]  5,  189,  '52.) 

POTASSIUM    CHLORATE    KC1O3. 

SOLUBILITY  IN  WATER. 

(Gay-Lussac  —  Ann.  chim.  phys.  n,  314,  1819;  Pawlewski  —  Ber.  32,  io4o,r>99;  above  100°,  Tilden 

and  Shenstone  —  Proc.  Roy.  Soc.  35,  345,  '81;  see  also  Blarez  —  Compt.  rend.  112,  1213,  '91; 

Etard — Ann.  chim.  phys.  [7]  2,  526,  94;  at  99°,  Kohler  —  Z.  anal.  Chem.  18,  242,  '79.) 

Gms.  KClOg  per  100  Gms.  0  Gms.  KClO.-<  per  TOO  Gms. 


c    . 

Solution. 

Water. 

Solution. 

Water. 

O 

3-04 

3.14 

3-3* 

70 

22-55 

29.16 

32-5* 

IO 

4.27 

4-45 

5-o 

80 

26.97 

36.93 

39-6 

2O 

6.76 

7  .22 

90 

31-36 

46.11 

47-5 

25 

7.56 

8.17 

8.6 

100 

35-83 

55-54 

56.0 

30 

8.46 

9.26 

IO.I 

120 

42.4 

73-7 

73-7 

40 

n-75 

I3-31 

14-5 

I36 

49-7 

98-5 

99.0 

50 

15.18 

17-95 

19.7 

I9O 

64.6 

183.0 

183.0 

60 

18.97 

23.42 

26.0 

330 

96.7 

2930-00 

* 

Gay  Lussac. 

POTASSIUM    CHLORATE 


240 


SOLUBILITY    OF    POTASSIUM    CHLORATE    IN   AQUEOUS    SOLUTIONS    OP 
POTASSIUM  BROMIDE  AT  13°. 

(Blarez  —  Com pt.  rend.  112,  1213,  '91.) 


Cms.  per  100  Cms. 
Solution. 

Gms.  per  100  Gms. 
Solution. 

Gms.  per  100  Gms. 
Solution. 

'KBr. 

KC1O3. 

KBr. 

KC1O3. 

KBr. 

KC103. 

O.2O 

5.l8 

I  .0 

5-04 

6.0 

3-46 

O-6o 

5.20 

2  -O 

4.60 

8.0 

2.8o 

0.8 

5.06 

3-o 

4.2 

10.  0 

2.40 

4-0 

4.0 

SOLUBILITY    OF    POTASSIUM    CHLORATE    IN   AQUEOUS    SOLUTIONS    OF 
OTHER  POTASSIUM  SALTS  AT  14°-!  5°. 

(Blarez.) 


Salt. 

KOH 
KC1 

KBr 
KI 

u 


Gms.  per  100  Gms.  Solution. 


K  Salt. 

KC1O3. 

4-47 

I.9I 
3-82 

4-45 
3-58 

3-05 

6.10 

4-49 
3.60 

4-25 
8.51 

4-59 
3-65 

Gms.  per  100  Gms.  Solution, 


oau.         <- 

K  Salt. 

KC103. 

KNO3 

2-59 

4-51 

u 

5.18 

3.88 

K^SO, 

2.23 

4.71 

U 

4.46 

3-98 

K2C2O4 

2.42 

4-72 

" 

4-85 

3-93 

SOLUBILITY    OF    POTASSIUM    CHLORATE    IN   AQUEOUS    SOLUTIONS    OP 
POTASSIUM  CHLORIDE  AT  20°. 

(Winteler  —  Z.  Electrochem.  %  360,  'oo.> 


p.  Gr.  of 

Grar 

ns  per  Liter. 

Sp  Gr.  of 

Gran 

is  per  Liter. 

olutions. 

KC1. 

KC103. 

Solutions. 

KC1- 

KC1O3. 

.050 

0 

7I.I 

I  .098 

120 

24-5 

•  050 

10 

58.0 

I.IOS 

I4O 

22  .5 

.050 

20 

49-0 

I.II9 

1  60 

21  .O 

•054 

40 

39-5 

I.I30 

180 

20.  o 

.064 

60 

34-o 

I  .140 

200 

20.  o 

•075 

80 

30.0 

1.168 

250 

20.  o 

.086 

100 

27.0 

SOLUBILITY    OF    POTASSIUM    CHLORATE    IN   AQUEOUS    SOLUTIONS    OF 
POTASSIUM  NITRATE. 

(Arrhenius  —  Z.  physik.  Chem.  n,  397,  '93.) 


Results  at  19.85' 


Results  at  23.87' 


Mols.  per  Liter. 

Grams  per  Liter.               Mols.  per  Liter. 

Grams  per  Liter. 

KN03.          KC103.  " 

KNO3. 

KC1O3       '  KNO3.        KC1O3' 

KN03.            KC103. 

o.o        0.570 

o.o 

69.88         o.o       0.645 

o.o         79-09 

0.125       0.529 

12.65 

64.86           0.5         0.515 

50.59         63.14 

0.25         0.492 

25.29 

60.33 

i.o        0.374 

ioi  .19 

45  .85 

2.O            0.328 

202.38 

40.22 

241 


POTASSIUM    CHLORATE 


SOLUBILITY  OF  POTASSIUM  CHLORATE: 

(Taylor  —  J.  Physic.  Chem.  i,  720,  '96- '97;  see  also  Gerardin  —  Ann.  chim.  phys.  [4]  5,  148,  '65.) 


In  Aqueous  Alcohol. 


In  Aqueous  Acetone. 


Wt.  percent           A^3O°- 
Alcohol  or    Gms.  KC1O3  per 
of  Acetone          «*>  Gms. 

At  40°. 
Gms.  KC1O3  per 
TOO  Gms. 

»  — 

At  30°. 
Gms.  KC1O3  per 
100  Gms. 

At  40°. 
Gms.  KC1O3  per 
100  Gms. 

insolvent.  Solution 

.     Water. 

Solution. 

Water. 

Solution. 

Water. 

Solution. 

Water. 

0 

9-23 

IO.I7 

12.23 

13-93 

9-23 

IO.I7 

11.23 

*3-93 

5 

7.72 

8.80 

10.48 

12-33 

8.32 

9-56 

II  .10 

13.11 

10 

6-44 

7-65 

8.84 

10-77 

7.63* 

9.09 

10.28* 

12  .60 

20 

4-51 

5-90 

6.40 

8.56 

6.09 

8.10 

8.27 

II  .26 

30 

3.21 

4-74 

4.67 

7-00 

4-93 

7.40 

6.69 

10.24 

40 

2-35 

4.00 

3-41 

5.88 

3-90 

6.76 

5-36 

9-45 

50 

i  .64 

3-33 

2.41 

4-94 

2.90 

5-98 

4-03 

8.40 

60 

I  .01 

2-53 

I.4I 

3-69 

2.03 

5-i7 

2.86 

7-35 

70 

o-54 

1.82 

0.78 

2.63 

1.24 

4.18 

1.68 

5.68 

80 

0.24 

I  .22 

0-34 

i-73 

o-57 

2.88 

0.79 

3-97 

90 

0.06 

O.62 

O-I2 

1.17 

0.18 

1.82 

0.24 

2-45 

*  Solvent,  9.09  Wt.  per  cent  Acetone. 

ioo  grams  glycerine  dissolve  3.5  grams  KC1O3  at  15.5°. 

100  grams  sat.  solution  of  KC1O3  in  glycol  contain  0.9  gram  KC1O3. 

(de  Coninck  —  Bui.  acad.  roy.  Belgique,  359,  '05.) 

POTASSIUM    (Per)    CHLORATE    KC1O4. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOL. 

(Muir  —  Chem.  News,  33,  15,  '76;  Wenze  —  Z.  angew.  Ch.  5,  691,  '91.) 


In  Water.     (M.) 


In  Alcohol.     (W.) 


t«. 

Gms.KClO4per 
ioo  Gms.  H2O. 

Sp.  Gr.  of 
Solutions. 

Wt.  per  cent     Gms.KClO4per 
Alcohol.      ioo  Gms.  Alcohol. 

6 

0-7 

I  .OOO5 

97-2 

0.0156 

25 

oo 

1-9 

6-45 

20.  0 

I.OI23 
I  -Ol8l 
I  .  0660 

95-8 
90.0 

O-020 
0-036 

POTASSIUM    CHLORIDE    KC1. 

SOLUBILITY  IN  WATER. 


Ver.  Zuckerind.  47,   447,   '97;  Andrae  —  J.  pr.  Chem.  [2]  29, 
[4]  5,  i37,   '65;  de  Coppet  Ibid.  [5]  3<>,  4".  '83;  Etard  Ibid.  [7] 
and  Shenstone  —  Proc.  Roy.  Soc.  (Lond.)  35,  345,  '83.) 

A0    Gms.  KC1  per  ioo  Gms.         ^0    Gms.KCl  per  ioo  Gms. 

456,   '84;  Gerardin  —  Ann.  chim.  phys. 
2,526,  '94;  Mulder;  above  100°,  Tilden 

i0         Gms.KCl  per  ioo  Gms. 

Solution. 

Water. 

Solution. 

Water. 

Solution. 

Water. 

-9 

19 

•3 

23-9 

40 

28, 

6 

40 

.0 

147 

41-5 

70.8 

-4-5 

20 

.6 

25-9 

So 

29 

9 

42 

.6 

180 

43-7 

77-5 

0 

21 

.6 

27-6 

60 

31 

3 

45 

•5 

Solid  Phase 

Ice 

5 

22 

•7 

29-3 

70 

32 

,6 

48 

•3 

-9 

19-3 

23-9 

10 

23 

•7 

31.0 

80 

33 

,8 

51 

.i 

-8 

.     17.7 

21-5 

15 

24 

•5 

32-4 

90 

35 

.1 

54 

.0 

-8 

16.7 

20.  0 

20 

25 

•4 

34-o 

IOO 

36 

.2 

56 

•7 

-7 

14.9 

J7-5 

25 

26 

.2 

35-5 

130 

39 

.8 

66 

.0 

-6 

13.6 

J5-7 

30 

27 

.1 

37-o 

-5 

•5  I2-5 

14-3 

Sp.  Gr.  of  solution  sat.  at  o  =  °i.iso;-  at  15°  =  1.172, 


POTASSIUM    CHLORIDE 


242 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  AMMONIUM 
CHLORIDE  IN  WATER  AT  25°. 

(Fock  — Z.  Kryst.  Min.  28,  353,  '97.) 


Grams  per  Liter 
Solution. 

Mol.  per  cent 
in  Solution. 

Sp.  Gr.  of 

oolutions* 

Mol.  per  cent  in 
Solid  Phase. 

'  NH4C1. 

KCl. 

NH4C1. 

KCl. 

NH4C1. 

KCl. 

o.oo 

311  .3 

o.oo 

100.  0 

1.1807 

o.o 

100 

22.  Si 

293-3 

9.41 

90.59 

i  .1716 

I  .21 

98.79 

35-39 

278.7 

15.04 

84.96 

1.1678 

2  -II 

97.89 

89.17 

273.2 

34.26 

65-74 

i  .1591 

6.18 

93.82 

127.8 

234.6 

46  •  59 

53-44 

1-1493 

8.90 

91.10 

147.2 

204.2 

5!-63 

48.37 

i  .1461 

10-53 

89.47 

197-3 

157-7 

63-56 

36-44 

i  .1391 

17.86 

82.14 

232-5 

116.8 

73-49 

26.51 

1.1326 

6o.20 

39.80 

244-5 

123.0 

73-48 

26.52 

1.1329 

76.88 

23.12 

261  .9 

in  .0 

79.10 

20.90 

1.1245 

97-51 

2-49 

259.0 

102  .2 

82.14 

17.86 

I  .1212 

97-79 

2  .21 

278.6 

53-16 

87.96 

12  .04 

I  •  IOO9 

98.85 

I  .15 

320.7 

3x-24 

93-45 

6-55 

I  .0912 

99-33 

0.67 

273-5 

o.oo 

100.00 

o.oo 

1.0768 

IOO-0 

o.oo 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  POTASSIUM 

BROMIDE  AT  25°. 

(Fock.)    . 


Grams  per  Liter 
Solution. 

Milligram  Mols. 
per  Liter. 

Mol.  per  cent     o     r*  ^f 

KPl    i'n                    "P-  "JP.OI 
£1  m          cAi«*;x^« 

Mol.  per  cent 
KCl  in 

KBr. 

KCl. 

KBr. 

KCl. 

Solution. 

Solid  Phase. 

558.I 

O-OO 

4686.2 

o.o 

o.o 

1-3756 

O.OO 

531-5 

23-44 

4462  .  7 

314.2 

6.16 

1.3700 

o.oo 

503-6 

46.57 

4228.5 

624.3 

12.86 

1.3648 

8.23 

454-6 

82.62 

3817.8 

1108.0 

22.49 

1-3544 

15.68 

379-6 

136.6 

3188.1 

1830.7 

36.48 

i-332o 

33-66 

324-8 

166.9 

2727.6 

2237.4 

45.06 

1.3119 

63-51 

218.0 

213.9 

1830.2 

2868.0 

60.30 

1.2689 

82.29 

140.7 

250.9 

1181.1 

3363-9 

74-oi 

1-2455 

88.04 

47-5 

291.7 

398.8 

39IJ-4 

85.22 

1.1977 

96.98 

o-o 

3*1-3 

o.o 

4173  -1 

100.00 

1.1756 

100  .  oo 

SOLUBILITY    OF    POTASSIUM    CHLORIDE    IN 
HYDROCHLORIC  ACID 

(Jeannel  —  Compt.  rend.  103,  381,  '86;  Engel  —  Ann 


AQUEOUS    SOLUTIONS    OF 

AT    0°. 

.  chim.  phys.  [6]  13,  377,  '88.) 


Milligram  Mols. 

per  10  cc.                  Grams  per  100  cc.  Solution.     Sp.  Gr.  o 

KCl. 

HC1. 

KCl. 

HCl.              Solutions 

34-5 

o.o 

25-73 

O-O 

•159 

30.41 

3-9 

22  .69 

1.42 

•^ 

27-95 

6.6 

20-84 

2-41             ] 

.150 

27-5 

7-1 

20.51 

2-59            3 

•  147 

23-75 

II  .1 

17.71 

4-05 

•137 

16.0 

23.0 

n-93 

8.39             I.  Ill 

10.0 

34-o 

7.46 

12.40            I-IO5 

7-5 

41  .0 

5  -60 

14.95             I-I05 

2  .0 

65-5 

1.49 

23.88             I.  121 

2-4 

148.8  (sat.) 

i-52 

54.26             1.224 

ioo  cc.  saturated  HCl  solution  dissolve  1.9  grams;  KCl  at  17°. 

(Ditte  —  Compt.  rend.  92,  ±42,  '86.) 


243  POTASSIUM    CHLORIDE 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  POTASSIUM 
HYDROXIDE  SOLUTIONS. 

(Engel  —  Bull.  soc.  chim.  [3]  6,  16,  '91;  Winteler  —  Z.  Electrochem.  7,  360,  'oo.) 

Results  at  o°.  Results  at  20°. 

(Engel.)  (Winteler.) 


Mg.  Mols.  per 
10  cc.  Solution           Sp.  Gr.  of 

Gms.  per  100  cc. 

Solution. 

Gms.  per  100  cc. 
Solution. 

Sp.  Gr.  of 

•Solution. 

KCl. 

KOH. 

KCl. 

KOH. 

kci. 

KOH. 

35-5 

O 

i 

•159 

26.83 

o 

.0 

29 

•3 

I  -O 

1.185 

3I.O 

2 

•375 

i 

.146 

23-44 

I 

•33 

21 

.1 

10.  0 

i  .210 

28.3 

4 

•7 

i 

•153 

21.39 

2 

.64 

14 

.8 

2O-O 

1.245 

23.0 

9 

•9 

i 

.172 

*7-39 

5 

•56 

10 

•4 

30.0 

1.295 

18-38 

15 

.1 

i 

.195 

13.89 

8.46 

6 

.8 

4O.O 

I-345 

14-43 

20 

•  o 

i 

.2l6 

10.91 

ii 

•23 

4 

.0 

5O.O 

1-397 

"•43 

24 

•63 

i 

•239 

8.64 

13 

•83 

2 

.2 

6o.O 

1.450 

8.98 

29 

•25 

i 

.26l 

6.78 

16 

•43 

I 

•4 

7O.O 

i  .500 

6.28 

35 

.13 

L 

.294 

4-74 

19 

•72 

1 

.1 

8o.O 

•i  .550 

O 

•9 

85.0 

1.580 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  POTASSIUM 

IODIDE  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  3,  275,  '94.) 
Grams  per  100  Gms.  Solution.  Grams  per  100  Gms.  Solution. 


I/  «B 

KCl. 

Kl. 

(/  • 

KCl. 

KI. 

0 

3-7 

50-5 

100 

6.2 

61  .0 

20 

4.2 

53-o 

140 

7-3 

63-7 

40 

4-7 

55-3 

180 

8-3 

65-5 

60 

5-2 

57-5 

220 

9-4 

66  3 

80 

5-7 

59-4 

245 

10.  0 

66.5 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  MAGNESIUM 
CHLORIDE  SOLUTIONS. 

(Precht  and  Wittgen  —  Ber.  14,  1667,  *8i.) 
Grams  KCl  per  100  Grams  Sat.  Solution  in: 


f. 

MII% 

15% 

MgCl2. 

21-2% 

MgCl*. 

30% 
MgCl2- 

20%  MKC1 

10 

14-3 

9-9 

5 

•3 

1-9 

4 

.2 

KC1+5 

7 

NaCl 

20 

*5-9 

6 

•5 

2.6 

6 

.0 

"   +5 

9 

" 

30 

17  .5 

12.7 

7 

.6 

3-4 

6 

•9 

"   +6 

.0 

" 

40 

19.0 

14.2 

8 

.8 

4.2 

7 

-9 

"  +6 

.1 

" 

50 

20.5 

15.6 

10 

.0 

5.0 

8 

•9 

"   +6 

•3 

11 

60 

21.9 

17.0 

ii 

.2 

5-8 

9 

•9 

"   +6 

•4 

" 

80 

24-5 

19-5 

13 

.6 

7-3 

10 

•9 

"   +6 

.6 

tt 

90 

25-8 

20.8 

14 

•7 

8.1 

ii 

•9 

"   +6 

•7 

" 

100 

27.1 

22.1 

15 

•9 

8.9 

13.0 

"   +6 

•9 

a 

POTASSIUM    CHLORIDE 


244 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  NITRATE,  AND  OF  POTASSIUM  NITRATE  IN  AQUEOUS 
SOLUTIONS  OF  POTASSIUM  CHLORIDE,  AT  SEVERAL  TEMPERATURES. 

(Touren  —  Compt.  rend.  130,  908 


1.  130,  908,  'oo;  Bodlander  —  Z.  physik.  Ch.  7,  360,  '91;  Nicol  —  Phil.  Mag. 
(Lond.)  31,  369,  '91;  Soch  — J.  Physic.  Ch.  2,  46,  '98.) 

KC1  in  Aq.  KNO3  Solutions  at: 


14-5°  (T.). 


17-5°  (B.). 


25.2°  (T.).         20°,  etc.  (N.). 


Gms.  per  Liter          <-     p_ 
Senior,               <*£££. 

Gms.  per  Liter. 

Gms.  per  Liter. 

Gms.  per  1000  Gms. 
H20. 

KN03. 

KCl. 

'KN03. 

KCI: 

KN03. 

KCI: 

KNO3l         KCI. 

0 

288 

•3 

•173 

0. 

0 

293-9 

0. 

0 

311 

.8 

o.oo    345.2 

20.64 

284 

.2 

.198 

65. 

8 

275.0 

13- 

76 

306 

.6 

56.18      342.15 

32.18 

282 

.  I 

.  2IO 

88. 

3 

273-4 

32. 

18 

303 

.6 

168.54      334.39 

62.  23 

276 

.8 

.225 

124. 

8 

265-3 

91. 

26 

293 

.2 

at  25° 

82.77 

273 

•5 

.236 

148. 

3 

259.8 

122. 

7 

287 

.2 

oor*     &         *J  AT      *) 

JI5-9 

270 

•  7 

•239 

152. 

2 

259.6 

141. 

4 

284 

.  2 

*^5-°     64L*6 

119.1 

268 

•3 

•239 

i54. 

9 

259-5 

182. 

7 

276 

.0 

at  80° 

123.4 

267 

.2 

.241 

153. 

3 

262.4 

1175.0      402.0 

KNO3  in  Aq.  KCl  Solutions  at : 
25-2°. 


Grams  per  Liter  Solution.  Grams  per  Liter  Solution.  Grams  per  1000  Gms. 


KCl. 

0.0 

I3-58 

3!-63 
65.64 
132.6 
164.4 
196.5 
236.9 


KN03. 
225.4 
219.8 
208.2 
185.2 

IS9-S 
J53-3 
144.0 


KCl. 
0.0 

19-39 
49.22 

IOO-7 

155-2 
207.3 
226.8 


KN03. 

325-5 
3*2-3 

288.7 

254.0 
224.4 
203.9 
196.9 


KCL 

o.o 

82.9 
165.8 
248.7 
310.8 


KNO3.  ' 

311.1 

256.8 
221-7 
202.  O 
501.6 


KNO3  in  Aq.  KCl  at  20.5°  (B.).         KCl  in  Aq.  KNO3  at  20.5°  (B.). 


Gms.  per  100  Gms. 
Solution. 

Sp.Gr.of 

O     1      i* 

KCl.                KN03. 

Solutions. 

o.o           27.68 

1.1625 

4.72            24.39 

I  .1700 

7-74            22.44 

1.1765 

12.23            20  -23 

1.1895 

15.15             18.96 

I.I983 

I9.6l             17.67 

I  .2150 

22.17             I7.II 

I  .2265 

24.96        16  79 

I  .  2400 

Gms.  per  100  Gms. 
Solution. 

Sp.  Gr.  of 

O1      A* 

KNO3. 

KCl. 

bolutions. 

o.o 

29-39 

1.1730 

6.58 

27.50 

i  .  1980 

8.88 

27-34 

I.  2100 

12.48 

26.53 

1.2250 

14.83 

25.98 

1.2360 

15.22 

25,96 

1.2390 

15-49 

25-95 

1.2388 

15-33 

26.24 

I.24IO 

245  POTASSIUM    CHLORIDE 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  CHLORIDE  AND  POTASSIUM 
SULPHATE  IN  WATER. 

Gms.  per  100  Gms,  Gms.  per  TOO  Gms. 
t°.                H20.                                  Observer.                          t°.  H2O.  Observer. 

KC1.     +     K2SO4.  KC1     +     K2SO4. 

10  30.9         I    32  (Precht  and  Wittgen.)  40  38.7       1.68  (P.  and  W.) 

15.8      28.0         2.3  (Kopp.)  50  41.3       1.82 

20  33-4          1-43  (pandW.)  6O  43.8       1.94 

2  5  34 -?6      2>93  (Van'tHoffand  Meyerhoffer.)       80  49-2       2.21  " 

30  36.1          1-57  (P.andW.)  100  54.5       2.53 


SOLUBILITY    OF    MIXTURES    OF    POTASSIUM    CHLORIDE    AND    SODIUM 
CHLORIDE  IN  WATER, 

(  (i)  Precht  and  Wittgen  —  Ber.  14,  1667,  '81;  at  25°  and  at  80°,  (3)  Soch  —  J.  Physic.  Ch.  2,  46,  '98; 
(2)  Etard  —  Ann.  chim.  phys.  [7]  3,  275,  '97.) 

0  Grams  per  100  Grams  H2O.  Grams  per  100  Grams  H2O. 

KCl Nad.  '  'KC1.  NaCl.  ' 

o  11.2(1)11.2(2)  30.0(030.0(2)   50  22.0(1)19.0(2)  27.7(1)32.3(2) 
10  12.5  12.3   29.7  30.5     60  24.6  20.6   27.2  32.8 

20  14-7  *3-8  29-2  3I-o  7o  27-3  32-5  26-8  34-1 

25  15.8(3)14.5  29.0(3)31.3  80  30.0(3)25.2(3)  26.4(3)34.0 

30  17.2  15.4  28.7  31.5  90  32.9  28.4  26.1  32.3 

40  19.5  17.0  28.2  31.9  100  34.7  32.3  25.8  30.6 

NOTE.  —  Page  and  Keightly,  Rudorff  and  also  Nicol,  give  single 
determinations  which  lie  nearer  the  results  of  Precht  and  Wittgen 
than  to  those  of  Etard. 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  CHLORIDE,  AND  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLU- 
TIONS OF  POTASSIUM  CHLORIDE,  AT  20°. 

(Nicol  — Phil.  Mag.  (Lond.)  31.  369,  '91-) 

KC1  in  Aq.  NaCl  Solutions.  NaCl  in  Aq.  KC1  Solutions. 

Grams  per  100  Grams  H2O.  Grams  per  100  Grams  HaO. 

'  NaCl.  KC1.     '  KC1.  NaCl. 

o.o  34-52                            °-°  35-91 

6-5  29.37                            4-H  34-39 

13.0  4-71                            8-29  32-7! 

19.5  .42  12.42  3I-3° 

100  gms.  40  per  cent  by  wt.  alcohol  dissolve  5.87  gms.  KC1  +  12.25 
gms.  NaCl  at  25°. 

100  gms.  40  per  cent  by  wt.  alcohol  dissolve  5.29  gms.  KNO3  +  10.06 

gms.  KC1  at  2 5°.  (Soch  —  J.  Physic.  Ch.  2,  46,  '98.) 

100  eras   r'  s.  ethyl  alcohol  dissolve  0.034  gm.  KC1  at  18.5°. 
100  'gins.  aos.  methyl  alcohol  dissolve  0.5  gm.  KC1  at  18.5°. 

(de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '92;  Rohland  —  Z.  anorg.  Ch.  18,  327,  '98.) 


POTASSIUM    CHLORIDE 


246 


SOLUBILITY  OP  POTASSIUM  CHLORIDE  IN  AQUEOUS  ALCOHOL. 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  140,  '65.) 

Interpolated  from  the  original  results. 

Grams  KC1  per  100  Gms.  Aq.  Alcohol  of  Sp.  Gr.: 


t°. 

0.9904 

0.9848 

0.9793 

0.9726 

0-9573 

0-939 

0.8967 

0.8244 

=  5-5 

=  9-35 

=  13.6 

=  19.1 

=  30 

=  40 

=  60 

=  90 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

Wt.%. 

o 

23-4 

19-5 

15-5 

«-S 

7-0 

4.0 

i-7 

o.o 

5 

25.0 

21  .O 

j6.8 

12.8 

8.0 

4-8 

2.2 

o.o 

10 

26.4 

22-5 

18.0 

14.0 

9.0 

5-6 

2-7 

o.o 

15 

26.8 

24.0 

19.2 

15.2 

IO.O 

6.4 

3-i 

0.04 

20 

29.1 

25-3 

20.3 

16.1 

10.8 

7.2 

3-5 

0.06 

25 

30-4 

26.8 

21.5 

17.1 

ii.  6 

7-9 

3-9 

0.08 

30 

31-? 

28.0 

22  .6 

18.2 

12.5 

8-5 

4.2 

O-IO 

40 

34-3 

30-8 

24.8 

20.  o 

14.0 

9-9 

4.8 

0.20 

50 

37-o 

33-5 

27.0 

21.8 

15-5 

10.8 

5-2 

0.30 

60 

16.8 

ii.  8 

5-5 

0.40 

SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  ALCOHOL  AT: 


(Schiff  —  Liebig's  Ann.  118,  365,  *6i.) 


14-5    • 
(Bodlander  —  Z.  physik.  Ch.  7,  316,  '91.) 


Sp.  Gr.          Wt.       G.  KCl  per 
of             per  cent     100  s.  Aq. 

Sp.  Gr. 
of  Sat. 

Grams  per  TOO  cc.  Solution. 

Alcohol.       Alcohol.      Alcohol. 

Solutions. 

C2H5OH. 

H20. 

KCl. 

0.984        10 

19. 

8 

I 

.1720 

. 

88 

.10 

29. 

10 

0.972             20 

14. 

7 

I 

.1542 

2 

•79 

85 

.78 

26. 

85 

0.958            30 

10. 

7 

I 

•1365 

4 

.98 

84 

.00 

24. 

67 

o  .  940        40 

7- 

7 

I 

.IO75 

10 

•56 

79 

.63 

20. 

56 

0.918            50 

5- 

o 

I 

.1085 

15 

•57 

75 

.24 

17- 

24 

0.896            60 

2  . 

8 

I 

•0545 

20 

.66 

70 

•52 

14. 

27 

0.848            80 

o. 

45 

I 

•0455 

24 

•25 

67 

•05 

13- 

25 

Gerardin's  results  at  15 

0  agree 

0 

•9695 

40 

.42 

5° 

.18 

6. 

35 

well  with  the 

above  deter- 

0 

•9315 

48 

•73 

40 

.60 

3- 

82 

minations. 

0 

.8448 

68 

•63 

15 

•55 

o. 

3o 

30 

0  and  40°. 

(Bathrick  —  J.  Physic.  Chem.  i, 

1  60, 

'96.) 

Wt. 

Gms.  KCl  . 

per  100  Gms. 

Wt. 

Gms. 

KCl  per  100  Gms. 

per  cent 

Aq.  Alcohol. 

per  cent 

Aq.  Alcohol. 

Alcohol. 

At  30°. 

At  40°. 

Alcohol. 

At  30°. 

At 

40°. 

0 

38.9 

41.8 

43 

.1 

II 

.1 

13 

.1 

5-28 

33-9 

35-9 

55 

•9 

6 

.8 

8 

.2 

9-43 

30.2 

33-3 

65 

•9 

3 

.6 

4 

.1 

16.9 

24.9 

27  .6 

78 

.1 

i 

•3 

I 

.0 

25.1 

19.2 

21.8 

86 

.2 

0 

•4 

0 

•5 

34-i 

15-6 

17.2 

247 


POTASSIUM    CHLORIDE 


SOLUBILITY  OF  POTASSIUM  CHLORIDE  IN  AQUEOUS  ACETONE 

SOLUTIONS. 

(Snell  — J.  Physic.  Ch.  2,  484.  '98;  at  20°,  Herz  and  Knoch  — Z.  anorg.  Ch.  41,  317,  '04.) 


Per  cent 

At   20°. 

At  30°. 

At  40°. 

At  50°. 

Acetone 
in 

KC1  per  100  cc. 
Solution. 

Gms.  per  100  Gms. 
Solution. 

Gms.  per  100  Gms. 
Solution  . 

Gms.  per  100  Gms. 
Solution. 

Solvent. 

Millimols.      Grams. 

Acetone.       KC1. 

Acetone.       KC1. 

Acetone.        KC1. 

O 

410.5        30.62 

o.   o     27.27 

o.o       28.69 

o.o        30.0 

9.1 

351.7        26.23 

6.96      23.42 

6-79      25.33 

... 

2O 

286.6        21.38 

l6.22       18.90 

15.75  ~21.28 

...               ... 

30 

223.7        16.69 

25.45       15.06 

two  layers 

25.67         14.42 

40 

166.5        12.42 

35-52       II-3I 

it 

36.03           9.93 

50 

115.4       8.61 

45.98         8.04 

d 

46.46           7.07 

60 

71-2        5-3i 

56.91          5.12 

(i 

57-37        4-38 

7° 

38.5        2.87 

68.18         2.60 

(t 

68.56             2.22 

80 

12.9       0.96 

78.43         0.76 

79-34      0.58 

79.25            0.94 

90 

2.O           O.I5 

89.88         0.13 

89.84      0.16 

8i°  +  sat.sol. 

100 

0.0           0.0 

100.  0            0.00 

100.00         0.00 

NOTE.  —  For  the  20°  results  the  per  cent  acetone  in  the  solvent  is 
stated  in  terms  of  volume  per  cent,  and  the  concentration  of  the  second 
solution  is  10  per  cent  instead  of  9.1  which  is  the  concentration  of  the 
solvent  for  the  corresponding  results  at  the  other  temperatures. 


AT  THE  TEMPERATURE  40°  AND  FOR  CONCENTRATIONS  OF  ACETONE 
BETWEEN  20  AND  80  PER  CENT  THE  SATURATED  SOLUTION  SEPAR- 
ATES INTO  Two  LAYERS  HAVING  THE  FOLLOWING  COMPOSITIONS: 


Upper  Layer. 

Grams  per  100  Grams  Solution. 


HjjO. 

(CH3)2CO. 

KCl. 

55-2 

31.82 

12.99 

53-27 

35-44 

ii  .29 

5*-23 

48.50 

10.27 

50-3  + 

39.88 

9-77 

48.02 

43.18 

8.79 

46.49 

45-34 

8.17 

58-99 

25.24 

15-77 

Lower  Layer. 

Grams  per  100  Grams  Solution. 


H2O. 

(CH3)2CO. 

KCl. 

28.14 

69.42 

2-44 

30.96 

65-97 

3-07 

32.64 

63-79 

3-56 

34-07 

62  .01 

3-92 

37-44 

57-67 

4.89 

38.68 

56-I7 

5-25 

23.66 

74.91 

i-43 

TOO  cc.  sat.   solution  of  potassium  chloride  in  furfurol  (C4H3O.COH) 
contain  0.085  gm-  KCl  at  25°. 

(Walden  —  Z.  physik.  Ch.  55,  713, '06.) 


POTASSIUM    CHLORIDE 


248 


SOLUBILITY    OF    POTASSIUM    CHLORIDE    IN    AQUEOUS    SOLUTIONS    OP 
GLYCERINE  AT  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Ch.  45,  267,  '05.) 

Sp.  Gr.  of  Glycerine  at  2  5 °/4°  =  1.2555.  Impurity  about  1.5%. 


Wt.  per  cent 
Glycerine  in 
Solvent. 

0 
13.28 
25.98 
4S-36 

KC1  per  100  cc. 
Solution. 

Sp.  Gr.  of 

Solutions. 

I.lSo 
1.185 
I.I94 
I.  211 

Wt.  per  cent        K.C1  per  100  cc. 
Glycerine  in             Solution 

Sp.  Gr.  of 
Solutions. 

I  .219 
1.259 
1.286 

Millimols.    Grams. 
424.5      31.66 
383.4      28.61 

339-3     25.31 
271.4    20-24 

Solvent.     Millimols.      Grams. 
54.23       238.5       17.79 
83.84       149.0       I  I.  I  I 

100.00     no.  6      8.25 

ioo  grams  H2O  dissolve  246.5  grams  sugar  +  44.8  grams  KC1  at 
31.25°,  or  ioo  grams  of  the  sat.  solution  contain  62.28  grams  sugar 
+  11.33  grams  KC1. 

(Kohler  — Z.  Ver,  Zuckerind.  47,  447,  '97.) 


POTASSIUM    CHROMATE    K2CrO4. 


POTASSIUM    (Di)    CHEOMATE    K2Cr2O7. 

SOLUBILITY  OF  EACH  IN  WATER. 

(Alluard  —  Compt.  rend.  59,  500,  '64;  Nordenskjold  and  Lindstrom  —  Pogg.  Ann.  136,  314, '69; 
Etard  —  Ann.  chim.  phys.  [7]  2,  527,  '94;  Kremers  —  Pogg.  Ann.  92,  497,  '54;  Tilden  and  Shenstone 
—  Phil.  Trans.  23,  1884.) 


Potassium  Chromate. 

Grams  per  ioo  Grams  Water. 


Potassium  Di  Chromate. 


o 

58.2* 

10 

60.0 

20 

61  .7 

25 

62.5 

30 

63  .4 

40 

65.2 

50 

66.8 

60 

68.6 

70 

70.4 

80 

72.1 

90 

73-9 

IOO 

75-6 

I25 

79.0 

150 

83.0 

S9-3t 

60.2* 

61  .2 

62.5 

63.2 

64-5 

64.2 

64-5 

65.2 

66.5 

67.0 

68.6 

69.0 

70.6 

71.0 

72.7 

73-o 

74-8 

75-o 

76.9 

77.0 

79.0 

79.0 

82.2 

Grams  per  ioo  Grams  Water. 

5* 

5§ 

7 

7 

12 

12 

16 

16 

20 

20  . 

26 

27 

34 

37 

43 

47 

52 

58 

61 

70 

70 

82 

80 

97 

no 

145 

143 

205 

Etard, 


t  Alluard. 


t  N.  and  L. 


§  A.,  K.,  T.  and  S. 


249 


POTASSIUM    CHKOMATE 


SOLUBILITY  OF  POTASSIUM  CHROMATES  IN  WATER  AT  30°. 

(Schreinemaker  —  Z.  physik.  Ch.  55,  83,  '06.) 


Composition  in  Wt.  per  cent  of: 


The  Solution. 

The  Residue. 

Per  cent  CrO3. 

Per  cent  K2O. 

Per  cent  CrO3. 

Per  cent  K2O. 

O 

±47 

o.o 

47.16 

12.59 

47-54 

0-1775 

34.602 

10-93 

37-47 

I-351 

26.602 

16.482 

32-532 

20.584 

37-I3I 

39.922 

I5-407 

19.225 

27.966 

29.377 

20.67 

19.17 

19.096 

17.30 

37-64 

22  .6l 

ii  .35 

7.88 

17-93 

3.412 

25-85 

7/82 

43  -51 

3.01 

49-45 

9.91 

44.46 

3-245 

53-94 

12.40 

46.368 

2.823 

60.314 

12-935 

49-357 

2-353 

63.044 

11.684 

53-215 

1.360 

62.958 

8.002 

62-55 

0.796 

67.944 

6.731 

62.997 

0.621 

70.0 

4.0 

62.28 

o.o 

.  .  . 

Solid 
Phase. 

KOH.2H20 
KaCrO, 


K2Cr04+K2Cr207 
K2Cr207 


K2Cr207  +  KaCraOjo 
K2Cr3010 


K2Cr4Ol3+Cr03 
CrOa 


ioo  gms.  sat.  solution    in  glycol  C2H4(OH)2.H2O    contain  1.7  gms. 
K2CrO4  at  15.4°. 

ioo  gms.  sat.  solution  in    glycol  C2H4(OH)2.H2O    contain  6.0  gms. 


7  at  14-6 


(de  Coninck  —  Bull.  acad.  roy.  Belgique,  257,  '05.) 


POTASSIUM    CITRATE    C3H4(OH)(COOK)3.H2O. 

SOLUBILITY  IN  WATER  AND  IN  SATURATED  SUGAR  SOLUTION  AT  31.25°. 

(Ko'hler  —  Z.  Ver.  Zuckerind.  47,  447,  '97.) 

ioo  gms.  H2O  dissolve  169.7  gms.  C6H5O7K3,  or  ioo  gms.  sat.  solu- 
tion contain  6  1  .  1  1  gms. 

ioo  gms.  H2O  dissolve  198.3  gms.  CCH5O7K3  -f  303.9  gms.  sugar, 
or  ioo  gms.  sat.  solution  contain  32.83  gms.  C6H5O7K3  4-  50.3  gms. 
sugar. 

POTASSIUM  CYANATE  KCNO. 


SOLUBJLITY    IN    ALCOHOLIC    MIXTURES. 
(Erdmann  —  Ber.  26,  2439,  '93.) 
Solvent. 

80  per  cent  Alcohol  +20  per  cent  Water 

80  per  cent  Alcohol  +   20  per  cent  Methyl  Alcohol 

80  per  cent  Alcohol  +  10  per  cent  Acetone 


Grams  KCNO  per 

Liter  Solvent  at  b.  pt. 

62 

76 

82 


POTASSIUM    CYANIDE    KCN. 

ioo  gms.  H2O  dissolve  122.2  gms.  KCN,  or  ioo  gms.  sat.  solution 
contain  55.0  gms.  KCN  at  103.3°.  (Griffiths.) 

ioo  gms.  abs.  ethyl  alcohol  dissolve  0.87  gm.  KCN  at  19.5°. 

ioo  gms.  abs.  methyl  alcohol  dissolve  4.91  gms.  KCN  at  19.5°. 

(de  Bruyn  —  Z.  physik,  Ch.  10,  783,  '92.) 

ioo  gms.  glycerine  dissolve  32  gms.  KCN  at  15.5°. 


POTASSIUM    CYANIDES  250 

POTASSIUM    CHEOMOCYANIDE    K3Cr(CN)6. 

100  gms.  H2O  dissolve  32.33  gms.  K3Cr(CN)6  at  20°. 

(Moissan  —  Ann.  chim.  phys.  [6]  4,  136,  '85;  Christensen  —  J.  pr.  Ch.  [2]  31,  166/85.) 


POTASSIUM    CHEOMISULPHOCYANIDE    K2Cr(SCN)6.4H2O. 
100  gms.  H2O  dissolve  139  gms.  salt. 

(Karsten  —  Ann.  Suppl.  3,  170.) 

POTASSIUM    CARBONYL    FERROOYANIDE  K3FeCO(CN)5.3iH2O. 
100  gms.  H2O  dissolve  148  gms.  salt  at  16°. 

(Miiller  —  Compt.  rend.  104,  992,  '87.) 

POTASSIUM    FEKBICYANIDE    K3Fe(CN)6. 


POTASSIUM    FEBROCYANIDE    K4Fe(CN)6.3H2O. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Wallace  — J.  Ch.  Soc.  7,  8°,  '85  ;  Etard  —  Ann.  chim.  phys.  [7]  2,  526,   '94;  Schiff  —  Liebig's  Ann. 
H3»  35°,  '60;  Michel  and  Krafft  —  Ann.  chim.  phys.   [3]    41,  478,  '58;  Thomsen.) 

NOTE.  —  The  available  determinations  fall  very  irregularly  when 
plotted  on  cross- section  paper,  and  the  following  figures,  which  are 
averages,  are  therefore  hardly  more  than  rough  approximations  to  the 
true  amounts.  The  figures  under  K4Fe(CN)6  show  the  limits  between 
which  the  correct  values  probably  lie. 

Grams  per  100  Gms.  H2O.  Grams  per  TOO  Gms.  H2O. 


t  . 
o 

10 
20 

25 
10 

K#e(CN)a.  K4Fe(CN)6. 

t". 

40 
60 
80 

100 
IQA.d 

K3Fe(CN)6.   K4Fe(CN)G. 

31 
36 

43 
46 

<0 

r3 

20 

25 
28 
32 

2O 

40 

48 

S7 

60 

66 
82.6 

38 
S2 
66 
76 

70 

83 
89 

9i 

POTASSIUM    FLUORIDE    KF.2H2O. 

100   gms.    H2O   dissolve   92.3    gms.  KF,  or   100   gms.  sat.  solution 
contain  48  gms.  KF  at  18°.     Sp.  Gr.  of  solution  =  1.502. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 

SOLUBILITY  OP  POTASSIUM  FLUORIDE  IN  HYDROFLUORIC  ACID  AT  21°. 

(Ditte  —  Compt.  rend.  123,  1282,  '96.) 
Gms.  per  100  Gms.  H2O.         Gms.  per  100  Gms.  H2O.  Gms.  per  100  Gms.  H2O. 


HF. 

KF. 

HF. 

KF. 

HF. 

KF.' 

o.o 

96-3 

9-2S 

29.9 

20.68 

38.4 

I  .21 

72.0 

II  .36 

29.6 

28.60 

46.9 

1.61 

61  .0 

12.50 

30-5 

41.98 

6l.8 

3-73 

40.4 

J3-95 

31-4 

53-71 

74-8 

4-03 

32-5 

15.98 

33-4 

74-20 

105.0 

6.05 

30-4 

17.69 

35-62 

119.20 

169.5 

POTASSIUM    FORMATE 


POTASSIUM    FORMATE    HCOOK. 


SOLUBILITY  OF  POTASSIUM  FORMATE  AND  OF  THE  ACID  SALT 

IN  WATER. 

(Groschuff  —  Ber.  36,  1785,  1903.) 


Solid  Phase  :  HCOOK 


Solid  Phase  :  HCOOK.  HCOOH. 


Gms. 
HCOOK 
t  °.         per  ioo 
Gms. 

Mols. 
HCOOK 
per  ioo 
Mols. 

Gms.  HCOOK      Gms. 
.HCOOH        HCOOK 
t  °.       per  ioo           per  ioo                t°. 
Gms.              Gms. 

Gms. 
HCOOK 
per  ioo 
Gms 

Mols. 
HCOOH 

Mol.1 

Solution. 

H20. 

Solution. 

Solution. 

Solution 

.   HCOOK. 

—     20 

72 

.8 

57 

•4 

0 

60 

•4 

39-o 

o 

36-3 

3-21 

4-  18 

76 

.8 

7i 

.0 

25 

69 

.8 

45-1 

19-5 

38.2 

2  .96 

50 

80 

•7 

89 

.8 

50 

79 

.2 

51.2 

39-3 

40.8 

2.65 

90 

86 

.8 

141 

.0 

80 

90 

•7 

58.6 

60 

44.0 

2-33 

120 

92 

.0 

247 

.0 

70 

45-9 

2.16 

I4O 

96 

.0 

511 

90 

52-1 

1.68 

157 

IOO 

.0 

00 

Sp.  Gr.  of  sat.  sol.  at  18°=  1.573. 

NOTE.  —  Since  the  acid  salt  is  less  soluble  at  ordinary  temperatures 
than  the  neutral  salt,  it  can  be  precipitated  from  the  solution  of  the 
neutral  salt  by  addition  of  aqueous  formic  acid.  Proceeding  in  this 
way  an  impure  product  is  obtained,  giving  solubility  values  (expressed 
in  HCOOK)  as  shown  in  the  last  three  columns  above. 

POTASSIUM    FLUOGERMANATE    K2GeF6. 
SOLUBILITY  IN  WATER. 

(Winkler;  Kruss  and  Nilson  —  Ber.  20,  1696,  '87.) 

ioo  gms.  H2O  dissolve  173.98  gms.K2GeF6  at  18°,  and  34-07  gms. 
at  100°  (W. ). 

ioo  gms.  H2O  dissolve  184.61  gms.  K2GeF6  at  18°,  and  38.76  gms.  at 
100°  (K.  andN.). 

POTASSIUM    HYDROXIDE    KOH. 

SOLUBILITY  IN  WATER. 

(Pickering  —  J.  Ch.  Soc.  63,  908,  '93;  at  15°,  Ferchland  —  Z.  anorg.  Ch.  30,  133,  '02.) 


Gms.  KOH 
t  °.            per  ioo  Gms. 

Solid 

Til  

t°. 

Gms 
per 

.  KOH 

TOO  Gms. 

Solid 
Phase. 

Water. 

Solution. 

Water.     Solution. 

—  22 

0 

•7 

3- 

6 

Ice 

15 

107 

51- 

7 

KOH.2H20 

—  20 

•7 

22 

•5 

18. 

4 

«« 

2O 

112 

S2- 

8 

" 

—  65 

.2 

44  -5     30  - 

8 

" 

30 

126 

55- 

76 

" 

-36 

.2 

36-2 

26. 

6 

KOH.4H2O 

32-5 

135 

57- 

44 

KOH.2H20  + 
KOH.H20 

—  32 

•7 

77 

•94 

43-8 

50 

140 

58. 

33 

KOH.H2O 

-33 

80 

44- 

4  KOH 

,4H20+KOH 

.2H20  IOO 

I78 

64- 

03 

41 

-23 

.2 

85 

45- 

9 

KOH.2H20 

I25 

2I3 

68, 

06 

M 

o 

97 

49  .  2 

143 

311 

•7  75 

73 

10 

103 

50 

•7 

" 

Sp.  Gr.  of  sat.  solution  at  15°  =  1.5355. 


POTASSIUM    IODATE  252 

POTASSIUM    IODATE   KIO3. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg.  Ann.  97t  5.  '56;  at  30°,  Meerburg  —  Ch.  Weekbl.  I,  474,  '04.) 
t°  0°         20°  30°  40°      60°  80°      100° 

Gms.  KIO3  per 

100  gms.  H2O      4.73     8.13     11.73     I2-8     J8-5     24.8     32.2 

100  gms.  H2O  dissolve  1.3  gms.  potassium  hydrogen  iodate(KH(IO3)2 

at  15°,  and  5.4  gms.  at  17°.  (Serullas  —  Ann.  chim.  phys.  22,  118.) 

ioo   gms.    H2O    dissolve   4.0   gms.   potassium   di   hydrogen  iodate 

KH2(IO3)2  at  1 5°.  (Meineke  —  Liebig's  Ann.  261,  360,  '91) 

POTASSIUM    IODIDE    KI. 

SOLUBILITY  IN  WATER. 

(Mulder;  de  Coppet^Ann.  chim.  phys.  [5]  30,  417,  '83;  Etard  —  Ibid.  [7]  2,  526,  '94;  Meusser  — 
Z.  anorg.  Ch.  44,  80,  05;  see  also  lilden  and  Shenstone  —  Phil.  Trans.  23,  '84;  Schreinemaker — 
Z.  physik.  Chem.  9,  71,  '92.) 


Gms,  KI  per  ioo  Gms. 

Gms. 

KI  per  ioo  Gms. 

t    , 

Water. 

Solution.                             r   • 

Water. 

Solution. 

—  10 

II5.I 

53 

•5 

80 

192 

65.8 

-  5 

II9.8 

54 

•5 

90 

2OO 

66.7 

—  i 

122  .2 

55 

.0 

IOO 

208 

67  5 

o 

127-5 

56 

.0 

no 

215 

68  3 

10 

I36 

57 

.6 

120 

223 

69  o 

20 
25 

144 
148 

59 
59 

.0 

•7 

Ice  Curve 

30 

152 

60 

•3 

-  5 

25 

•7 

22    5 

40 

1  60 

61 

•5 

-  7 

42 

.6 

29.9 

50 

1  68 

62 

•7 

-  9 

•5      51 

•5 

34-o 

60 

176 

63 

•7 

—  ii 

•5      64 

•7 

39-3 

70 

184 

64.8 

-14 

75 

.8 

427 

SOLUBILITY  OF  POTASSIUM  IODIDE  IN  ABSOLUTE  ALCOHOLS, 

(de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '92;  Rohland  —  Z   anorg.  Ch.  18,  327,  '98.) 

ioo  gms.  methyl  alcohol  dissolve  16.5  gms.  KI  at  20.5°. 

ioo  gms.  ethyl  alcohol  dissolve  1.75  gms.  KI  at  20.5°. 

ioo  gms.  propyl  alcohol  dissolve  0.46  gm.  KI  at  i5°-2o°  (R.). 

SOLUBILITY  OF  POTASSIUM  IODIDE  IN: 


Ethyl  Alcohol 

of  0.9496  Sp.  Gr. 

Aqueous  Ethyl  Alcohol  at  18°. 

*"" 

Gms.  KI  per 

Sp.  Gr. 

Weight 

Gms.  KI 

Sp.  Gr. 

Weight 

Gms.  KI 

t°. 

IOO 

of 

per  cent 

per  ioo  Gms. 

of 

per  cent 

per  ioo  Gms 

Gms.  Alcohol 

Alcohol. 

Alcohol. 

Alcohol. 

Alcohol. 

Alcohol. 

Alcohol. 

8 

67.4 

0.9904 

S-2 

I30-5 

0.9390 

45 

66.4 

I3 

69.2 

0.9851 

9.8 

119.4 

0.9088 

59 

48.2 

25 

75-1 

0.9726 

23.0 

IOO.  I 

0.8464 

86 

II-4 

46 

847 

0.9665 

29.0 

89.9 

0.8322 

9i 

6.2 

55 

87-5 

0.9528 

38.0 

76.9 

62 

90.2 

(Gerardin 

—  Ann.  chim.  phys.  [4]  5,  155,  '65.) 

253  POTASSIUM    IODIDE 

SOLUBILITY   OF   POTASSIUM   IODIDE   IN  ACETONE   AND  IN  PYRIDINE. 

(von  Laszcynski  —  Ber,  27,  2285,  '94;  at  25°,  Krug  and  McElroy  —  J.  Anal.  Ch.  6,  184,  '92.) 
Gms.  KI  per  100  Gms.  Solvent  at: 


Solvent.  , 

-2.5°.  10°.  22°.  25°.  S6°. 

Acetone        3  .08          ...          2.38         2.93         1.21 
Pyridine          ...          0.26 

100  gins,  glycerine  dissolve  40  gms.  KI  at  15.5°. 


SOLUBILITY  OF  POTASSIUM  IODIDE  IN  SEVERAL  SOLVENTS. 

(Walden  — Z.  physik.  Ch.  55,  714,  '06.) 


Solvent. 

Formula. 

t°. 

Sp.  Gr.  of 

Gms.  KI  per  TOO 

Solution. 

cc.  Solution. 

Gms.  Solution. 

Water 

H2O 

o 

I  .  6699 

94-05 

56-32 

Water 

H20 

25 

I-7254 

102.  70 

59-54 

Methyl  Alcohol 

CH3OH 

o 

o.  8964 

II.  6l 

12.95 

Methyl  Alcohol 

CH3OH 

25 

0.9003 

I3-5-I4. 

3       J4-97 

Ethyl  Alcohol 

C2H5OH 

o 

0.8085 

I.I97 

1.479 

Ethyl  Alcohol 

C2H5OH 

25 

o.  7908 

1.520 

1.922 

Glycol 

(CH,OH)2 

0 

1-3954 

43.28 

31-03 

Glycol 

(CH2OH)a 

25 

1.3888 

47-23 

33-oi 

Acetonitril 

CH3CN 

0 

0.8198 

1.852 

2.259 

Acetonitril 

CH3CN 

25 

o.  7938 

i-57 

2.003 

Propionitril 

C,H5CN 

0 

0.8005 

0.34-0. 

41      0.0429 

Propionitril 

C,H5CN 

25 

0.7821 

0.32-0. 

36      0.0404 

Benzonitril 

C6H5CN 

25 

i  .  0076 

0.051 

0.0506 

Nitro  Methane 

CH3NO2 

0 

i.  1627 

0.314-0 

.366  0.315 

Nitro  Methane 

CH3N02 

25 

1.1367 

0.289-0.349  0.307 

Nitro  Benzene 

C6H5N02 

25 

0.0019 

Acetone 

(CH3)2CO 

o 

0.8227 

1.732 

2.  105 

Acetone 

(CH3)2CO 

25 

o.  7968 

1.038 

1.302 

Furfurol 

C4H3O.COH 

0 

.  .  . 

15.  10 

.  .  . 

Furfurol 

C4H3O.COH 

25 

i.  2014 

5-93 

4*94 

Benzaldehyde 

C6H5COH 

25 

i  .  0446 

o-343 

0.328 

Salicyl  aldehyde 

C6H4.OH.COH 

o 

i.  1501 

1-257 

1.093 

Salicyl  aldehyde 

C6H4.OH.COH 

25 

I-I373 

0-549 

0.483 

Anis  aldehyde 

C6H4.OCH3.COH 

0 

1.1223 

1.520 

1-355 

Anis  aldehyde 

C6H4.OCH3.COH 

25 

1.1180 

0.720 

0.644 

Ethyl  Acetate 

CH3COOC2H5 

25 

0.0013 

Methyl  Cyan  Acetate 

CH2CNCOOCH3 

o 

i.  1521 

3-256 

2.827 

Methyl  Cyan  Acetate 

CH,CNCOOCH3 

25 

I-I358 

2-459 

2.165 

Ethyl  Cyan  Acetate 

CH2~CNCOOC2H5 

25 

1.0628 

0.989 

0.930 

POTASSIUM    NITRITE  254 

POTASSIUM    NITRITE    KNO2. 

100  gms.  H2O  dissolve  about  300  gms.  KNO2  at  15.5°. 

(Divers  —  J.  Ch.  Soc.  75,  86,  '99.) 

POTASSIUM    NITRATE    KNO3. 

SOLUBILITY  IN  WATER. 

(Mulder;  Andrae  —  J.  pr.  Ch.  [2]  29,  456,  '84;  Gerardin  —  Ann.  chim.  phys.  [4]  5,  150,  '65;  Etard  — 
Ibid.  [7]  2,  526, '04;  Ost  —  J.pr.  Ch.[>]i7,  233, '78;  at  31-25°.  Kphler  —  Z.  Ver.  Zuckerind.  47,  447, 
'97;  Euler  —  Z.  physik.  Ch-49,  315,  '04;  Tilden  and  Shenstone  —  Phil.  Trans.  23,  '84;Berkeley  —  Trans. 
Roy.  Soc.  203  A,  213,  '04.) 

Average  Curve. 

0  Gms.KNO3  per  100  Gms.  Gms.KNO3  per  TOO  Gms. 

Water.  Solution.  Water.  Solution. 

o  13.3  11.7  70  138  58.0 

10  20.9  17.3  80  169  62.8 

2O  3-1  •  6  24.0  90  202  66.9 

25  37.3  27.2  ioo  246  71.1 

30  45.8  31.4  no  300  75.0 

40  63.9  39.0  120  394  79.8 

50  85.5  44.0  125  493  83.1 

60  no.o  52.0 


SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  NITRATE  AND   BARIUM 
NITRATE  IN  WATER. 

(Euler  —  Z.  physik.  Ch.  49,  313,  '04.) 
t°.          Sp.  Gr.  of  Sat.  Solution.  Grams  per  ioo  Grams  H2O. 

17  1. 120  13.26  KNO3+  6.31  Ba(NO3)2 

21.5  17.00      "     +   7-58 

30  1.191  24.04  +  9.99 

50  49-34  +18.09 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  NITRIC 

ACID  AT  o°. 

(Engel  —  Compt.  rend.  104,  913,  '87.) 


p.  Gr.  of 

Equivalents  per  10  cc.  Solution. 
x 

Grams  per  ioo  cc.  Solution. 

1.079 

12 

•5 

KN03 

o 

HN03 

12 

•65 

KNO3 

O 

.00 

HN03 

9 

•9 

tt 

5 

.87      "    ' 

10 

.02 

" 

3 

7i 

tt 

1.093 

8 

.28     " 

13 

.2 

8 

•38 

" 

8 

38 

" 

.117 

7 

•4 

ii 

21 

•55      " 

7 

•49 

" 

13 

58 

tt 

.144 

7 

•4 

n 

3I.I                                      7.49 

a 

19 

47 

ii 

•  2O2 

7 

.6 

tt 

48 

•  o 

7 

.68 

u 

30 

.04 

n 

.289 

10 

•3 

ii 

68 

.0            " 

10 

.42 

tt 

42 

86 

n 

-498 

28 

•3 

tt 

120 

•5 

28 

.64 

u 

75 

95 

tt 

255 


POTASSIUM    NITRATE 


SOLUBILITY  OF  POTASSIUM  NITRATE  AND  OF  ACID  POTASSIUM  NITRATES 

IN  NITRIC  ACID. 

(Groschuff  —  Ber.  37,  1490,  '04.) 

NOTE.  —  Determinations  made  by  the  so-called  thermometric 
method,  i.e.,  by  observing  the  temperature  of  the  disappearance  of 
the  separated,  finely  divided  solid  from  solutions  of  known  concen- 
tration. 


t°. 

Grams 

per  100  Gms. 
Solution.                       Solid 

Gms.  per  i 
t  °.               Soluti 

oo  Gms. 
on. 

Solid 

TJU,.,.. 

KNO3. 

HN03. 

KN03. 

HN03.                  iliasc' 

-    6 

24 

•4 

75- 

41       KNO3.2HNO3  (i) 

22-5 

47-2 

52-93 

KNO3.HNO3 

+  14 

32.6 

67. 

42             "          (stabil) 

23-5 

47-8 

S2 

.11 

(stabil) 

17 

34 

8 

65- 

04 

25-5 

48.6 

51 

.46 

" 

19 

•5     37' 

2 

62. 

90 

27.0 

49-4 

So 

.78 

" 

22 

44- 

5 

55- 

46 

29.0 

50.1 

49 

•94 

KN03.HN03 

21 

•5     47- 

8 

52- 

1  1       KN03.2HN03  (2) 

30-5 

50-9 

49 

•!5 

(labil) 

21 

•5     48. 

6 

S1- 

46             "            (labil) 

21  -O 

49-4 

50 

•78 

KN03       (labil) 

20 

50. 

9 

49- 

IS 

39-o 

50-9 

49 

•J5 

(stabil) 

-    4 

37- 

2 

62. 

8  1        KN03.HN03 

50 

51.7     48.32 

-16 

•5     44-5 

55- 

46             "            (labil) 

C1) 

Solution  in  HNO3. 

(2)  Solution 

in 

KN03. 

CONDUCT 

OF 

ACID  POTASSIUM 

NITRATE  TOWARDS 

WATER. 

Gms.  per  100  Gms. 
t°.            Solution.                         .Sohd                             to. 

Gms.  per  100  Gms. 
Solution. 

Solid 
Phase. 

KNO3. 

HN03. 

KNO3. 

HNO3. 

22 

44- 

5 

55- 

5         KN03.2HN03 

5o 

38. 

7 

48. 

3 

KNOg 

2O 

•5     44- 

i 

55- 

o 

61 

36. 

0 

44- 

8 

" 

18 

43- 

8 

54- 

5 

63 

34- 

5 

43  -° 

12 

43- 

0 

53- 

6 

60.5 

30- 

9 

39-5 

6 

42. 

3 

52  • 

7 

56 

27. 

6 

34- 

4 

" 

0 

41. 

6 

S1- 

8 

43 

20. 

8 

25- 

9 

" 

12 

41. 

3 

S1- 

4         KN03 

17 

ii  . 

7 

16. 

6 

" 

22 

40. 

9 

S1- 

o 

-5 

5- 

54 

6. 

91 

" 

40 

39- 

9 

49- 

8 

SOLUBILITY   OF   MIXTURES   OF   POTASSIUM   NITRATE   AND   POTASSIUM 
CHLORIDE  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  3,  283,  '94;  at  20°,  Rudorff  —  Ber.  6,  482,  '73;  Nicol  —  Phil.  Mag.  [5] 

3it  385.  '91-) 


Gms.  per  100  Gms. 
t°.              Solution. 

Gms.  per  100  Gms. 
t°_              Solution. 

Gms.  per  100  Gm: 
^o                 Solution. 

KN03.       KC1. 

o      5.0     20.0 

10         8.0       20.8 
2O       12-6       21.2 
25       14.0       21-3 

KN03.         KC1. 
30       l6-O       21.2 
4O       21.0       2  1  -  O 

50     27.0     20.  o 

60      33-5       19-0 

KNO3.         KC1. 

7o    39-5     :7-5 
80    45-5     x5-8 
100     57.5     i  i  -6 

120      69.0         7-7 

POTASSIUM   NITRATE  256 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF: 

(Touren  —  Compt.  rend.  131,  259,  'oo.) 

Potassium  Carbonate.  Potassium  Bi  Carbonate. 

Results  at  14.5°.  Results  at  14.5°. 


Mols.  per  Liter 

Cms 

.  per  Liter. 

Mols.  per  Liter. 

Grams  per  Liter. 

K2C03 

KNU3. 

K2C03. 

KN03. 

KHC03. 

KN03.          KHC03. 

KN03. 

o.o 

2 

.228 

O 

•  O 

225 

O 

•  o 

2 

•33 

o.o 

236 

0.48 

I 

•85 

66 

•4 

188 

O 

•39 

2 

•17 

39-0 

2  2O 

1.25 

I 

•39 

172 

•9 

141 

O 

.76 

2 

•03 

76.0 

205 

2.58 

0 

.86 

356 

•9 

87 

I 

.16 

I 

.92 

116 

194 

3-94 

0 

.64 

544 

•9 

65 

I 

•55 

I 

.81 

155 

183 

Results  at 

25°. 

Results  at 

25°. 

o.o 

3 

.217 

O 

.0 

326 

0 

.0 

3 

.28 

o.o 

332 

o-59 

2 

.62 

81 

.6 

265 

0 

.89 

2 

.84 

89 

287 

i-35 

I 

•97 

186 

•7 

199 

I 

•33 

2 

•65 

133 

268 

2.IO 

I 

.46 

290 

•5 

148 

I 

.91 

2 

•45 

191 

249 

2.70 

I 

.14 

373 

.6 

"5 

3-58 

0 

•79 

495 

.1 

80 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  NITRATE  AND  POTASSIUM 
SULPHATE  IN  WATER. 

(Euler  —  Z.  physik.  Ch.  49,  313,  '04.) 
t°.  Sp.  Gr.  of  Sat.  Solution.  Grams  per  100  Grams  Water. 

15  1.165  24/12  KNO3  "    5.65  K2SO4 

20  30.10      "  5.58      " 

25  i. 210  36.12  5.58 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  NITRATE  AND  SODIUM 
CHLORIDE  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  3,  283,  '94;  the  older  determinations  of  Rudorff,  Karsten,  Mulder,  etc., 
agree  well  with  those  of  Etard.) 

Gms.  per  100  Gms. 
*  °  Solution . 


t°. 

Gms.  per  100  Gms. 
Solution.                     t°. 

Gms.  per  100  Gms. 

Solution. 

KN03. 

NaCl. 

KN03- 

NaCl." 

0 

13 

24 

40 

30.5 

19 

10 

16 

23 

50 

36 

20 

20 

22 

60 

42-5 

15 

25 

23 

21-5 

80 

,55 

12 

30 

25 

20-5 

IOO 

67 

9-5 

KNO3.  NaCl. 

120    73  8.0 

140   77  7.0 

i 60    79.5  6.0 

170   80.5  5.5 


SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
NITRATE  AND  VICE  VERSA  AT  20°. 

(Carnelly  and  Thomson  — J.  Ch.  Soc.  53,  782,  '88;  Nicol  — Phil.  Mag.  31,  369,  '91.) 

KNO3  in  Aq.  NaNO3  Solutions.        NaNO3  in  Aq.  KNO3  Solutions. 

Grams  per  100  Grams  H2O.  Grams  per  TOO  Grams  H2O. 

NaN03.  KN03  KNO3.      '  NaNO3. ' 

o  31.6  o  88 

10  30.5  10  90 

20  31.0  20  92 

40  33-0  25  93 

6o  35-5  30  94 

80  41.0  35  96 


257  POTASSIUM    NITRATE 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  NITRATE  AND  SILVER  NITRATE 

IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  3,  283,  '94.) 


Gms.  per  100  Gms.  Sol. 

^  0        Gms.  per  100  Gms.  Sol. 

0       Gms.  per  100  Gms.Sol. 

' 

KN03. 

AgN03. 

KN03. 

AgNU3. 

' 

KN03. 

O 

13-5 

43 

•  o 

30 

26 

.8 

49-4 

80 

36.2 

55 

.1 

10 

19.0 

44 

•7 

40 

29 

.6 

51  .5 

IOO 

38.3 

55 

•3 

20 

23.0 

47 

.0 

50 

32 

.0 

54-o 

120 

4O.O 

55 

.6 

25 

25.0 

48 

.0 

60 

33 

•5 

54-8 

140 

41-5 

55 

.8 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  NITRATE  AND  SILVER 
NITRATE  IN  WATER  AT  25°. 

(Herz  — Inaug.  Diss.  (Berlin)  '05;  Calc.  by  Fock  —  Z.  Kryst.  Min.  28,  405,  '97.) 


Grams 

per  Liter. 

Mg.  Mols. 

per  Liter. 

Mol.  per  cent 
AgN03  in 
Solution. 

Mol.  per  cent 
AgN03  in 
Solid  Phase. 

AgNOg. 

KN03. 

AgN03. 

KN03. 

45-9 

321.8 

•270 

3l8o 

7-83 

0-2896 

110.7 

322  .6 

651  .3 

3^4 

16.96 

o  .  6006 

176.8 

333-7 

1040 

3298 

23-97 

o  .  9040 

259.6 

364.0 

1528 

3597 

29.81 

1.054 

365  .6 

456-4 

2151 

4511 

32.28 

I  .604 

5°7-9 

387.2 

2988 

3816 

43.85 

2-439 

745-9 

398.6 

4388 

3960 

52.70 

8.294 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  NITRATE  AND  THAL- 
LIUM NITRATE  IN  WATER  AT  25°. 

(Fock.) 


Grams  per  Liter. 

Mg.  Mols. 

per  Liter. 

Mol.  per  cent 
TINOa 

Sp.  Gr. 
of 

Mol.  per  cent 
T1NO3 

T1NO3. 

KN03. 

T1N03. 

KN03. 

in  Solution. 

Solutions. 

in  Solid  Ph;sj. 

0-00 

35J-o 

o.o 

3468.2 

o.oo 

I  .2632 

O-OO 

2-37 

329.0 

8.9 

325I-5 

o-43 

I.I903 

0.08 

6-15 

332-4 

23.1 

3285.1 

0.70 

I.I956 

0-20 

17.64 

333-7 

66.3 

3298.1 

1.97 

I  .2050 

o-57 

49-74 

333-3 

186.9 

3294.4 

5-37 

I  .2196 

1.78 

63.60 

321.0 

239.0 

3*72-4 

7.01 

1.2436 

2  .19 

86.18 

330-5 

323-8 

3265-8 

9.02 

I  .2617 

2-77 

123.8 

428.3 

465.2 

4232.6 

9.90 

1.2950 

|    6.00 
1  27.04 

101.3 

245.1 

380.6 

2423-3 

I3-58 

I  .2050 

93-33 

116.1 

o.o 

463.1 

o.o 

100.00 

I  .0964 

100-00 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  ALCOHOL  SOLUTIONS. 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  151,  '65.) 
Grams  KNO3  per  100  Grams  Aqueous  Alcohol  of  Sp.  Gr.: 


t  o 

1  — 

0.9904 

0.9843 

0.9793 

0.9726 

•09571 

0.939 

0.8967 

0.8429 

wts%. 

=  13-6 

Wt.%. 

=  19.1 

Wt.%. 

=30 

Wt.%. 

=40 

Wt.%. 

=  60 
Wt.%. 

=90 

Wt.%. 

10 

17 

13 

10 

7 

4-5 

3 

I 

0-2 

18 

22-5 

i8.5 

14.5 

10 

6.2 

4-5 

1.6 

o-3 

20 

24 

20 

16 

ii 

7-o 

5 

2 

o-3 

25 

29 

24-5 

20 

13.5 

9.0 

6-5 

2-5 

0.4 

30 

36 

30 

25 

17 

ii  .5 

8 

3-o 

o-5 

40 

S2 

43 

36 

27 

16.5 

ii 

4 

0.6 

50 

72 

61 

50 

38 

23.0 

16 

6 

0.7 

60 

93 

79 

69 

52 

31-0 

21 

8 

i  .1 

POTASSIUM    NITRATE  258 

SOLUBILITY  OF  POTASSIUM  NITRATE  IN  AQUEOUS  ALCOHOL  AT  18°. 

(Bodlander  —  Z.  physik.  Ch.  7,  316,  '91.) 

Sp.  Gr.  of        Gms.  per  100  cc.  Solution.  gp.  Gr.  of        Gms.  per  IOQ^CC.  Solution. 

Solution.        C2H6OH.       iSx  KNO3.  Solution.  C2H6OH.         ScT KNO3. 

.1480          ...          89.80       25.0  I.OI2O  23.33       69.81       8.06 

.1085          3.30      87.44       20.11  0.9935  28.11       64.74      6.50 

.1010  5.24  86.26  18.60  0.9585  37.53  54-21  4.11 

.0805  8.69  83.18  16.18  0.9450  42.98  48.15  3.37 

•0755  9-°6  83-Jo  15-39  0.9050  51.23  27.32  1.95 

.0655  14.08  77.93  14-54  0.8722  61.65  24.74  0.83 

1.0490  16.27  76-36  12.27  0.8375  69.60  13-95  0-20 

!-o375  J9-97  72-93  !o-85 

SOLUBILITY  OF  POTASSIUM   NITRATE  IN  AQUEOUS  ALCOHOL  AND  IN 
AQUEOUS  ACETONE. 

(Bathrick  — J.  Physic.  Ch.  i,  160,  '96.) 

In  Aqueous  Alcohol.  In  Aqueous  Acetone  at  40°. 

W«,  Percent      G-f-^O- 


Wt.  per  cent 

jms.  JsJNUa  per  100  ^r 

,x_. 

ms.  AQ.  Aiconoi 

Alcohol.         ' 

At      °            "* 

0 

45-6 

64-5 

8.25 

32-3 

47.1 

17.0 

22.4 

33-3 

25-7 

^S-1 

24.1 

35-o 

11.4  (34-4°) 

16.7 

44-9 

7.0 

11-6(44°: 

54-3 

4-5 

7-2(55°: 

65.0 

2-7 

4-4 

75-6 

i-3 

2.0  (76. 

88.0 

0.4 

0.6  (88. 

o  64.5 

8.5  51.3 

16.8  38.9 

25  .2  22  .8 

34.3  24.7 

44-i  17-0 

53-9  "-9 

64.8  7.2 

76.0  3.0 

.5°)        87.6  0.7 

100  grams  H2O  saturated  with  sugar  and  KNO3  dissolve  224.7  gms- 
sugar  +  41  .  9  gms.  KNO3,  or  100  gms.  of  the  saturated  solution  contain 
61.36  gms.  sugar  +  11.45  gms-  KNO3  at  31.25°. 

(Kohler  —  Z.  Ver  Zuckerind.  47,  447,  '97.) 

POTASSIUM    OXALATE    K2C2O4.4H2O. 

SOLUBILITY  OF  MIXTURES  OF  POTASSIUM  OXALATE  AND  OXALIC  ACID 

IN  WATER  AT  25°. 

(Foote  and  Andrew  —  Am.  Ch.  J.  34,  155,  '05.) 
Gms.  per  100  Gms.  Solution.          Mols.  per  100  Mols.  H2O. 

'H2C204.     *        K2C20;.  'H2C204.      '       K2C204:  Solid  Phase. 

10-2  ...  2.274  ...  Hj!C2O4.2H2O 

10.31  O.O4  2.302  O-CO1?  H2C2O4.2H2O  +  H3K(C2O4)2-2H2O 

2.046  0.016  DoublesaltH3K(C204)2.2H20 


3-39  °-63  0.707  0.071 

2.o6  4.26  O  -  440  O  .  49  5              H3K(C2O4)  -2H2O  +  HKC2O4 

I.I6  11.50  0.266  1.427          {DoublesaltHKC20, 

0.99  io-93  0.240  2.235       * 

0.85  2  1.  08  0.221  2.928              HKC204  +  H2K4(C204)3.2H20 

0.82  21-49  0.2II  2.998         "] 

0.64  23.52  O.I  69  3-3^1           [•  Double  salt  H2K4(C2O4)3.2H2O 

0.57  24.88  0.153  3.617       j 

°-43  27'52  0.122  4.14                H2K4(C204)3.2 

27.40  ...  4.09  K2C204.H20 


259 


POTASSIUM    OXALATE 


SOLUBILITY  OF  POTASSIUM  OXALATE  AND  ACID  POTASSIUM  OXALATE  IN 

WATER. 

(Alluard;  results  at  o°,  Engel  —  Ann.  chim.  phys.  [6]  13,  362,  '88.) 

ioo  gms.  H2O  dissolve  25.24  gms.  K2C2O4,  or  100  gms.  of  sat.  solu- 
tion contain  20.62  gms.  K2C2O4  at  o°.     Sp.  Gr.  of  solution  =  1.161. 


Acid  Oxalate  in  Solutions  of  Neutral  Oxalate  at  o°. 


Acid  Oxalate  in  Water 


»  H2SO4  Corre- 
sponding to  K 
in  10  cc.  Sol. 

n  KOH  Corre- 
sponding to  Free 
Acid  in  10  cc. 

Sp.  Gr.  of 
Solutions. 

Gms. 

TOO  CC 

per 

t  °. 

Gms.  KHC204 
per  ioo  Gms. 

K2C204. 

H2C264.                                  n2U- 

28. 

5 

0-4 

I  . 

164 

23 

•53 

o, 

18 

O 

2 

.2 

10. 

8 

0.925 

8 

.91 

O 

,41 

10 

3 

.1 

6, 

8 

1-075 

I 

042 

5 

.61 

O 

,48 

20 

5 

.2 

4- 

78 

1.25 

I  , 

031 

3 

•94 

O 

•56 

40 

10 

•5 

3- 

83 

i-45 

I 

025 

3 

.16 

O 

•65 

60 

20 

•5 

3- 

35 

I 

,022 

2 

.76 

0 

.68 

80 

34 

•7 

2  . 

6(1) 

1-85 

I 

.Ol8 

2 

0 

•83 

IOO 

51 

•5 

2. 

o  (2) 

2.25 

I 

.007 

I 

•65 

I 

.00 

o. 

45(3) 

1.25 

I 

•  004 

O 

•37 

O 

•56 

(i)   Sat.  with  acid  potassium  oxalate. 


(2)  Sat.  with  both  acid  oxalate  and  tetroxalate. 


(3)  Sat.  with  tetroxalate. 

POTASSIUM    PERMANGANATE    KMnO4. 

SOLUBILITY  IN  WATER. 

(Baxter,  Boylston,  and  Hubbard  —  J.  Am.  Ch.  Soc.  28,  1343,  '06  ;  Patterson — Ibid.  28,  1735,  '06.) 


Grams  KMnO4  per  ioo  : 


Grams  KMnO4  per  ioo  : 


Gms.  Solution 

.     Gms.  H2O 

.   cc.  Solution  (P). 

Gms.  Solution. 

Gms.  H20. 

O 

2-75 

2.83 

2.84 

34-8 

9.64 

10.67 

9-8 

4-13 

4.31 

.  .  . 

40 

II  .l6 

12.56 

15.0 

5.22 

45 

12-73 

14.58 

19.8 

S-96 

6-34 

50 

14-45 

16.89 

24.8 

7  .06 

7  59 

.  .  . 

55 

16.20 

19-33 

29.8 

8.28 

9-03 

8.69 

65 

20.02 

25-03 

Sp.  Gr.  of  saturated  solution  at  15°  =  1-035. 

SOLUBILITY  OF  POTASSIUM  PERMANGANATE  IN: 

Water.  Aqueous  Acetone  Solutions  at  13 


(Voerman  —  Chem.  Centrb.  77,  I,  125,  '06.) 


(Herz  and  Knoch  —  Z.  anorg.  Ch.  41,  317  '04.) 


t°. 

Gms.  KMnO4  per 
ioo  Gms.                 Solid 

cc.  Acetone       KMnO4  per  ioo  cc. 
oer  ioo  cc.               Solution. 

Solution. 

Water. 

Solvent. 

Millimols. 

Grams. 

—  0.18 

0-58 

0.58             Ice 

0 

148.5 

4.70 

-  0.27 

o-99 

1.  01 

10 

l62  .2 

S'*3 

-  0.48 

1.98 

2.02 

2O 

177-3 

5.61 

-  0.58 

2  .91 

3  •  OO  Ice  +  KMnO4 

30 

208.2 

6-59 

+  10-  O 

4.01 

4-22        KMnO4 

40 

257-4 

8.14 

15 

4-95 

5-20 

50 

289.7 

9.16 

25 

7.00 

7-53 

60 

316.8 

IO-O2 

40 

10.40 

ii.  61 

70 

328.0 

10.38 

50 

14-35 

16.75 

80 

3I2-5 

9.89 

90 

227  .0 

7.18 

IOO 

67.0 

fl.14 

POTASSIUM    PERMAN-  260 

6ANATE 

SOLUBILITY  OF  MIXED  CRYSTALS  OP  POTASSIUM  PERMANGANATE  AND 
POTASSIUM  PERCHLORATE  AT  7°. 

(Muthmann  and  Kuntze  —  Z.  Kryst.  Min.  23,  368,  '94;  recalculated  by  Fock  —  Ibid.  28,  402,  '97.) 

Mol.  per  cent 
Milligram  Mols.  per  Liter.  Grams  per  Liter.  KMnO4  in 

KMnO4. KC1O3. '  KMnO4. KC1O4.  "  Crystals  of  Solid 

o.o  63.91  o.oo  8.86  o.oo 

29-37  54-48  4.65  7.55  2.84 

67.73  42-75  10.71  5.93  9-78 

79-04  39-59  12-50  5-49  Jo-8i 

99.81  38.63  15.79  5.36  15.96 

122.24  34-39  19-34  4-77  23.56      - 

119.21  38-91  18.84  5-39  24.28 

128.08  33-77  20.26  4.68  26.40 
144.46  33.14  22.86  4.59  34.32 

167.81  29.53  26.55  4-09  44-42 

183.09  25.19  28.97  3.49  67.33 

197.82  20.16  3I-3°  2.80  77-95 

233.75  28.26  36.98  3.92  94.37 
264.27               o.oo                41.81             o.oo                 100.00 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  PERMANGANATE  AND 
RUBIDIUM  PERMANGANATE  AT  7°. 

(Muthmann  and  Kuntze,  calc.  by  Fock.) 

Milligram  Mols.  per  Liter.  Grams  rjer  Liter.  KMnO4  in 

KMn04. RbMn04.  KMnO4-  RbMnO4'.  Crystals  of  Solid 

Phase. 

27.04  22.69  4.28  4.64  3.50 

75-00  22.22  11.84  4-54  13-75 

120.26  31-29       J9-o3     6.40       34-29 

188.30    38.98     29-80    7.97      71.45 
198.36    41.29     31.39    8.44      92.50 

205.76  42-50       32 .56     8.69       99-47 
225.12     26.00       35.61     5.32       99-32 

264.27  o.oo       41.81     o.oo       100.00 

POTASSIUM    PHOSPHATE    KH2PO4    (Monobasic). 
One  liter  aqueous  solution  contains  249.9  grams  at  7°. 

(Muthmann  and  Kuntze.) 

POTASSIUM    HYPOPHOSPHATE,  etc. 

SOLUBILITY  IN  WATER. 

(Salzer  —  Liebig's  Ann.  211,  i,  82.) 

Gms.  Salt  per  100 
.       Salt.  Formula.  Gms.  H2O. 

Cold!  Hot. 

Potassium  Hypophosphate  K4P2O6.8H2O  400 

Hydrogen  Hypophosphate  K3HP2O6.3H2O  200 

Di  Hydrogen  Hypophosphate  K2H2P2O6.3H2O      33  100 

Tri  Hydrogen  Hypophosphate  KH3P2O6                 66.6  200 

Penta  Hydrogen  Hypophosphate  K3H5(P2O6)2. 2H2O  40  125 

Hydrogen  Phosphite  KH2PO3  172  (20°)  . . . 

Hypophosphite  KH2PO2  200  (25°)  333 

Hypophosphite  KH2PO2*                 14.3(25°)  28 

*  Solvent  alcohol. 


26i  POTASSIUM    PHOSPHO- 

MOLYBDATE 
POTASSIUM    PHOSPHOMOLYBDATE    K3PO4.nMoO3.iiH2O. 

100  gms.  H2O  dissolve  0.007  gms-  at  30°. 

100  gms.  aqueous  10  %  HNO3  dissolve  0.204  gms.  at  30°. 

(Donk  —  Proc.  Assoc.  Official  Agrl.  Chemists  — Bull.  No.  90,  Bureau  of  Chemistry, 
U.  S.  Dept.  of  Agr.,  '05.) 

POTASSIUM    SELINATE    K2SeO4. 

SOLUBILITY  IN  WATER. 

t°.  -20°.        -5°.        +5°.  18°.          97°. 

Gms.  K2SeO4  per  100  gms.  solution     51-5     51-7     52.0     52.6     54.9 

(Etard  —  Ann.  Chim.  phys.  [7]  2,  550,  '94.) 

POTASSIUM    STANNATE    K2SnO3.3H2O. 

100    gms.  H2O   dissolve  106.6  gms.  at  10°,  and  110.5  gms-  a"t  20°. 
Sp.  Gr.  at  10°  =  1.618  at  20°  =  1.627. 

(Ordway  —  Am.  J.  Sci.  [2]  40,  173,  '65.) 

POTASSIUM    SULPHATE    K2SO4. 

SOLUBILITY  IN  WATER. 

(Mulder;  Andrae  —  J.  pr.  Ch.  29,456,  '84;  Trevor  —  Z.  physik.  Ch.  7,  468,  91;  Tildenand  Shenstone 
-—  Phil.  Trans.  31,  '84;  Berkeley  —  Trans.  Roy.  Soc.  203  A,  209,  '04;  see  also  Etard  —  Ann.  chim.  phys. 
17J  2,  549.  '94-) 


Gms.K2SO4per  looGms.       A0      Gms.  K2SO4  per  TOO  Gms. 

Gms.  K2SO4  per  loo  Gms. 

' 

Water. 

Solution. 

Water. 

Solution. 

' 

Water. 

Solution. 

O 

7-35 

6 

•85 

40 

14 

.76 

12 

.86 

90 

22.8 

18.57 

10 

9-22 

8 

•44 

5° 

16 

•50 

14 

16 

IOO 

24.1 

19.42 

20 

II  .11 

10 

.00 

60 

18 

•17 

15 

•38 

I2O 

26.5 

20-94 

25 

12  .04 

10 

•75 

70 

19 

•75 

16 

49 

143 

28.8 

22.36 

30 

12-97 

ii 

.48 

80 

21 

•4 

i7 

63 

170 

32-9 

24.76 

Sp.  Gr.  of  solution  saturated  at  18°  =  1.083. 

SOLUBILITY  OF  POTASSIUM  SULPHATE  IN  AQUEOUS  AMMONIA 
SOLUTIONS  AT  20°. 

(Girard  —  Bull.  soc.  chim.  [2]  43,  552,  '85.) 

Gms.  NH3  per  zoo  cc.  solution  o          6.086     15.37     24.69     31.02 

Gms.  K2SO4  per  loo  cc.  solution      10.80     4.10        0.83       0.14      0.04 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  SULPHATE  AND 
AMMONIUM  SULPHATE  AT  25°. 

(Fock  —  Z.  Kryst.  Man.  28,  375,  '97.) 


Grams  per  Liter. 

Milligram  Mols.  per  Liter. 

Mol.  per  cent 
K2S04  in 
Solution. 

Sp.  Gr. 
of 
Solution. 

Mol.  per  cent 
K2SO4  in 
Solid  Phase. 

K2SO4. 

(NH4)2S04. 

K2S04. 

(NH4)2S04. 

127.9 

O-O 

734 

o.o 

IOO 

1.  086 

IOO 

135-7 

115-7 

778.5 

874-6 

47-1 

I.I49 

91.28 

84.20 

281.1 

483 

2126 

18.5 

I  .2OO 

80.05 

59.28 

355-o 

340 

2685 

11.13 

I  .226 

68.63 

40.27 

482-7 

23I 

3650 

5-98 

I  .246 

27-53 

o.oo 

542-3 

O-O 

4100 

o.oo 

1.245 

o.oo 

Results  are  also  given  for  14°,  15°,  16°,  30°,  46°,  and  47°. 


POTASSIUM    SULPHATE  262 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  COPPER  SULPHATE 
AND  AMMONIUM  COPPER  SULPHATE  IN  WATER. 

CuSO4.K2SO4.6H2O  and  CuSO4(NH4)2SO4.6H2O  at  i3°-i4°. 

(Fock.) 

Mols.  per  100  Mols.  H2O     Mol.  per  cent  K  Salt         Mols.  per  icy  Mols.  H2O      Mol.  per  cent  K  Salt 
K.  Salt.         NH4  Salt,       in  Solution,    in  Solid.  K  Salt.        NH4  Salt,      in  Solution.        in  Solid. 

o-oo  1-035  o-00  °-°°  0.2946  0.5096  36.63  58.20 

0.0897  0.8618  5.06  10.34  0.3339  0.3319  50.15  75.34 

0.2269  0.6490  16.76  33-05  0.4560  0.1961  69.93  83.86 

0.2570  0.5887  30.40  46.22  0.4374  o.oo  100.00  100.00 


SOLUBILITY  OF  SOME  POTASSIUM  DOUBLE  SULPHATES  IN 
WATER  AT  25°. 

(Locke  —  Am.  Ch.  J.  27,  459,  '01.) 

Double  Salt.                                                Formula.  p^T^Gms?1 

Potassium  Cobalt  Sulphate        K2CO(SO4)2.6H2O  '        12.88 

Copper       "               K2Cu(SO4)2.6H2O  11.69 

Nickel        "               K2Ni(SO4),.6H2O  6.88 

"         Zinc            "               K2Zn(SO4)2.6H2O  13.19 


SOLUBILITY  OF  POTASSIUM  NICKEL  SULPHATE  AND  ALSO  OF  POTASSIUM 

ZINC  SULPHATE  IN  WATER  AT  DIFFERENT  TEMPERATURES. 

Grams  per  100  Gms.  H2O.  Grams  per  100  Grams  H^. 

*°-              '  K2Ni(SO4)2        K2Zn(SO4)2*  t0-                'K2Ni(SO4)2        K2Zn(SO4)2 

.6H2O.              .6H2O.  .6H2O.                .6HO2. 

o                  6                13  40                23                45 

10                  9                19  50                28                56 

20                14               26  60                35                72 

25                16                30  70                43                88 
3o                18               35 


SOLUBILITY  OF  THE  THREE  HYDRATES  OF  POTASSIUM  FERRO  SULPHATE 
IN  WATER  AT  DIFFERENT  TEMPERATURES. 

(Kuster  and  Thiel  —  Z.  anorg.  Ch.  21,  116,  '99.) 
K2S04.FeSp4.6H20.  K2SO4.FeSO4.4H2O.  K2SO4.FeSO4.2H2O. 


t°.     cc.N/ioKMnO4   Gms.  K2SO4  cc.N/ioKMnO4  Gms.K2SO4    cc.N/io  KMnO4  Gms.  K2SO' 

per  2cc. 
Solution. 

-FeSO4  per 
100  cc.  Sol. 

per  2  cc. 
Solution. 

.FeSO4  per 
100  cc.  Sol. 

per  2  cc. 
Solution. 

.FeS04per 
100  cc.  Sol. 

o-5 

12-4 

18.36 

*5-5 

22.94 

15-4 

22-79 

17.2 

17.0 

25  .16 

18.1 

26.79 

21  .6 

31.98 

40.1 

24-8 

36.72 

21  .9 

32.41 

27.6 

40.86 

60 

29.0 

42-93 

24.1 

35-68 

28.8 

42.63 

80 

30.6 

45-29 

27-3 

40.46 

28.6 

42-34 

90 

29.6 

43-82 

28.9 

42-73 

95 

29.8 

44.11 

27.7 

41  .01 

263 


POTASSIUM    SULPHATE 


SOLUBILITY  OF  POTASSIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OP 
POTASSIUM  CHLORIDE,  BROMIDE,  AND  IODIDE. 

(Blarez  —  Com pt.  rend.  112,  939,  '91.) 

Interpolated  from  the  original  results. 


Grams  Halogen 
Salt  per  100 
cc.  Solution. 


O 

2 

4 

6 

8 

10 

12 


Grams  K.2SO4  per  100  cc.  in  Aq. 
Solutions  of: 


KC1 

KBr 

KI 

at  12.5°. 

at  14°. 

at  12.5°. 

9-9 

10.  16 

9-9 

8-3 

9.1 

9.2 

7.0 

8.2 

8.4 

5-7 

7-4 

7-7 

4.6 

6.6 

7.2 

3-5 

6.0 

6.6 

5-5 

6.0 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  POTASSIUM  SULPHATE  AND 
POTASSIUM  CHROMATE  AT  25°. 

(Fock  —  Z.  Kryst.  Min.  28,  379,  '97.) 


Milligram  Mols.  per  Liter 

Grams  per  Liter. 

Mol.  pe 
K2SC 

r  cent          Sp.  Gr.      Mol.  per 

~>.  in                        of                        TC^O. 

cent 
in 

'   K2S04.        K2Cr04. 

K2S04. 

K2CrO4. 

Solution.            Solution.      Solid  P 

iase. 

618.1 

o 

.0 

107 

•7 

O 

.00 

100 

.O              1-083 

IOO 

•  O 

608.4 

103 

106 

.0 

2O 

.02 

85 

•51        i 

.092 

99 

•65 

341.0 

691 

.8 

59 

.46 

134 

•5 

33 

.01             I 

.141 

97 

•30 

174-8 

1496 

.0 

30 

•47 

290 

•5 

10 

.50            I 

.231 

91 

•97 

110.7 

2523 

19 

•30 

490 

•5 

4 

•2i         i-356 

28 

•43 

100-6 

2687 

17 

•54 

522 

•3 

3 

.60         1.377 

2 

.41 

o.o 

2847 

o 

•  o 

553 

•5 

0 

.00         1.398 

O 

.00 

734-o 

o 

.0 

127.9 

o 

.0 

100 

.0          1.0863 

IOO 

•  o 

617.0 

103 

•4 

107 

.6 

20 

.1 

85 

.65         1-0934 

99 

.78 

463 

452 

•7 

80 

.72 

88 

.0 

55 

•55 

•I235 

98 

•49 

279 

948 

.2 

48 

.64 

184 

•4 

22 

.72 

.1700 

96 

.07 

153 

1469 

26 

.68 

285 

.6 

9 

.41 

•2255 

85 

•77 

296 

2681 

51 

.61 

521 

.2 

21 

.09 

.3688 

25 

•73 

o.o 

2715 

o 

.00 

527 

.8 

O 

.00 

•378i 

o 

.00 

SOLUBILITY  OF  POTASSIUM  SODIUM  SULPHATES  IN  WATER. 


Double  Salt. 


3K2S04.Na2S04 
5K2SO4.Na2SO4 


4.4 
12.7 

IOO.O 


Cms.  per  100 
Cms.  H2O. 

40.8 

9.2 

10. 1 

25.0 


Authority. 

(Penny  —  Phil.  Mag.  [4]  10,  401,  '55.) 
(Gladstone  — J.  Ch.  Soc.  6,  n,  '54-) 


POTASSIUM    SULPHATE  264 

SOLUBILITY  OF  POTASSIUM  SULPHATE  IN  AQUEOUS  ALCOHOL. 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  147.  '65;  Schiff  —  Liebig's  Ann.  118,  362,  '61.) 

In  Aq.  Alcohol  of  0.939  In  Alcohol  of  Different 

Sp.  Gr.=  4o  Wt.  %.  Strengths  at  15°. 

Cms.  K2SO4  Weight  Cms.  K2SO4 

t°.  per  100  Gms.  per  cent  per  100  Gms. 

Alcohol.  Alcohol.  Sat.  Sol. 

40  0.16  10  3.90 

80  O.2I  2O  1.46 

60  0.92  30  0.56 

40  O.2I 

ioo  gms.  glycerine  of  1.255  Sp.  Gr.  dissolve  1.316  gms.  K2SO4  at  ord. 

temp.  (Vogel  — Neues  Report,  Pharm.  16,  557  '67.) 

SOLUBILITY  OF  POTASSIUM  SULPHATE.  IN  AQUEOUS  ACETIC  ACID  AND 
IN  AQUEOUS  PHENOL  SOLUTIONS  AT  25°. 

(Rothmund  and  Wilsmore  —  Z.  physik.  Ch.  40,  619,  '02.) 


In  Aq.  Acetic  Acid. 

Mols.  p^er  Liter.                Grams  per  Liter. 

In  Aq.  Phenol. 

Mols.  per  Liter.                     Grams  per  Liter. 

CH3COOH. 

K2S04. 

CHgCOOH 

.    K2S04. 

CeHsOH. 

K2S04. 

C0H5OH. 

K2S04. 

o. 

0 

0-6714 

O 

.0 

117.0 

O 

•  O 

O 

.6714 

0.0 

II7.0 

o. 

07 

0.6619 

4 

.2 

115.4 

O 

.032 

0 

.6598 

3-01 

II5.0 

o. 

137 

0-6559 

8 

.22 

114.4 

O 

.064 

0 

.6502 

6.  02 

IJ3-3 

o. 

328 

0.6350 

J9 

.68 

no.  8 

0 

.127 

o 

.6310 

11.94 

no.o 

o. 

578 

0.6097 

34 

.68 

106.3 

0 

.236 

o 

.6042 

22.19 

J°5-3 

I. 

151 

o-SSS6 

69 

.06 

96.87 

o 

.308 

0 

•5834 

28.97 

101  .7 

2  . 

183 

0-4743 

128 

•58 

82.70 

0 

.409 

o 

•5572 

38.46 

97.2 

o. 

464 

o 

.5480 

43-63 

95-5 

0.498  (sat.)  0.5377  46.82   93.8 

ioo  grams  water  dissolve  10.4  grams  K2SO4+  219.0  grams  sugar  at 
31.25°,  or  ioo  grams  sat.  solution  contain  3.18  grams  K2SO4  4-  66.74 

grams  SUgar.  (Kohler  —  Z.  Ver.  Zuckerind.  47,  447,  '97.) 

POTASSIUM    ACID    SULPHATE    KHSO4. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Liebig's  Ann.  92,  497,  '54.) 
t°  0°  20°  40°  100° 

Gms.  KHSO4  per  ioo  gms.  H2O          36.3         51.4        67.3         121.6 

POTASSIUM    PERSULPHATE    K2S2O8. 

ioo  gms.  H2O  dissolve  1.77  gms.  K2S2O8  at  o°. 

(Marshall  — J.  Ch.  Soc.  59,  77 1,  '91.) 

POTASSIUM    SODIUM    THIOSULPHATE    KNaS2O3.2H2O. 

POTASSIUM    SODIUM    HYDROGEN    SULPHITE       KNa2H(SO3)2. 
4H20. 

ioo  grams  H2O  dissolve  213.7  grams  KNaS2O3.2H2O  (a)  at  15°. 
ioo  grams  H2O  dissolve  205.3  grams  KNaS2O3.2H2O  (6)  at  15°. 
ioo  grams  H2O  dissolve  69.0  grams  KNa2H(SO3)2.4H2O  at  15°. 

(Schwicker  —  Ber.  22,  i73i»  '89.) 


20 


265  POTASSIUM    SULPHO- 

CYANIDE. 
POTASSIUM    SULPHOCYANIDE    KSCN. 

100  grams  H2O  dissolve  177.2  grams  K*SCN  at  o°,  and  217.0  grams  at 

(Rudorff  —  Ber.  2,  68,  '69.) 

SOLUBILITY  OF  POTASSIUM  SULPHOCYANIDE  IN  ACETONE,  AMYL 
ALCOHOL,  ETC. 

(von  Laszcynski  —  Ber.  27,  2285,  '94.) 

In  Acetone.     In  Amyl  Alcohol.     In  Ethyl  Acetate.     In  Pyridine. 


Gms.  KSCN  per              Gms.  KSCN  per                   Gms.  KSCN  per                 Gms.  KSCN  per 
t°.         100  Gms.             t°.         100  Gms.                t°.            100  Gms.               t°.         100  Gms. 

(CH3)2CO. 

CeHnOH. 

CH3COOC2H6. 

C&HsN. 

22 

20-75 

13 

0.18 

O 

0.44 

0 

6-75 

58 

20-40 

65 

i-34 

14 

0.40 

20 

6.15 

100 

2.14 

79 

0.20 

58 

4-97 

133-5 

3-15 

97 

3.88 

"5 

3.21 

POTASSIUM  (Bi)  TARTBATE  (Mono)  KHC4H4O6  Cream  of  Tartar. 
SOLUBILITY  OF  MONO  POTASSIUM  TARTRATE  IN  WATER. 

(Alluard  —  Liebig's  Ann.  133,  292,  '65;  Roelofsen  —  Am.  Ch.  J.  16,  466,  '94;  Blarez  —  Compt.  rend. 


112,  434,  '91;  at  20°,  Magnanini  —  Gazz.  chim.  ital.  31,  II,  542,  'or;  at  25°,  Noyes 
Z.  physik.  Ch.  13,  413,  '94.) 

and  Clement  — 

Gms.  KHCJ^Ofl 

Gms. 

KH 

C4H4O« 

per 

ioo  Gms.  Solution. 

t°. 

per  ioo 

Gms.  Solution. 

0 

o.3o(R. 

)  o 

•32  (A.) 

o-35(B.) 

40 

0.96 

I. 

3           I- 

29 

10 

0.37 

O 

.40 

0.42 

5° 

1.25 

I. 

8           I. 

80 

20 

0.49 

0 

•53  (M.) 

0.60 

60 

2. 

4 

25 

0.58 

0 

.654(N.  andC.) 

0.74 

80 

.... 

4- 

4 

30 

0.69 

o 

.9  (A.) 

0.89 

IOO 

6. 

5 

SOLUBILITY  OF  POTASSIUM  ACID  TARTRATE  (KHC4H4O6)  IN  NORMAL 
SOLUTIONS  OF  ACIDS  AT  20°. 

(Ostwald;  Huecke  —  J.  pr.  Ch.  [2]  29,  49.  '84-) 

Purified  tartrate  was  added  in  excess  to  normal  solutions  of  the  acids, 
and  after  shaking  clear  i  cc.  portions  of  each  solution  were  withdrawn 
and  titrated  with  approximately  N/io  Ba(OH)2  solution;  i  cc. 
normal  acid  requiring  10.63  cc-  °f  the  Ba(OH)2  solution. 


Acid. 

Gms. 
Acid 

cc.  N/io 
Ba(OH)2 

Gms. 
KHC,H406            A^ 

Gms.      cc.  N/io      Gms 
Acid     Ba(OH)2  KHC4H4O0 

per  roo  cc. 
Solvent. 

per  i  cc. 
Solution. 

per  IOQCC. 
Solution. 

per  loo  cc. 
Solvent. 

per  i  cc.  per  ico  cc 
Solution.     Solution' 

HN03 

6. 

31 

5 

.77* 

10 

.21 

C2H5S03H 

II 

.0 

5.01* 

8.87 

HC1 

3. 

65 

5- 

32 

9 

42 

HO.(CH2)2S03H 

12. 

61 

5-33 

9-43 

HBr 

8. 

10 

5- 

38 

9- 

75 

C6H5S03H 

15- 

81 

5-25 

9.29 

HI 

12. 

80 

5- 

43 

9- 

61 

HCOOH 

4- 

60 

0-45 

0.80 

H2S04 

4- 

90 

3- 

97 

7- 

03 

CH3COOH 

6 

00 

0.27 

0.48 

HCH3SO4 

ii. 

21 

5- 

58 

12. 

44 

CH2C1COOH 

9- 

45 

I.  01 

1.79 

HC2H5S04 

12. 

61 

5- 

4i 

9- 

58 

C2H5COOH 

7 

40 

o.  24 

0.42 

HC3H7S04 

14- 

01 

5- 

21 

9- 

22 

C3H7COOH 

8. 

81 

0.23 

0.41 

*  The  figures  in  this  column  show  the  amount  of  the  Ba(OH)2  solution  in  excess  of  that  which  would 
have  been  required  by  the  normal  acid  solution  alone  in  each  case,  viz.,  10.63  cc.  They,  therefore,  corre- 
spond to  the  amount  of  KHC^Oo  dissolved  in  i  cc.  of  each  saturated  solution,  and  when  multiplied 
by  i-77give  the  grams  of  KHC^Oo  per  100  cc.  solution. 


POTASSIUM    TARTRATE. 


266 


SOLUBILITY  OF  MONO  POTASSIUM  TARTRATE  (KHC4H4O6)  IN  AQUEOUS 
SOLUTIONS  OF  ELECTROLYTES  AT  25°. 

(Noyes  and  Clement  —  Z.  physik.  Ch.  13,  413,  '94;  Magnanini  —  Gazz.  chim.  ital.  31,  II,  542,  foi.) 


Cms. 

Equiv. 

Cms. 

per 

Gm. 

Equiv  . 

Grams 

per 

Electro- 

per 

Liter. 

100  CC. 

Electro- 

per  Liter. 

100  CC. 

lyte. 

Electro-   KHC4 

Electro- 

KHC* 

lyte. 

Electro-  KHC4  " 

Electro- 

KHC4' 

lyte. 

H406. 

lyte. 

H406. 

lyte. 

H406. 

lyte. 

H406. 

KC1 

0.025 

0.0254 

1.86 

0.4788 

CH3COOK 

0.05 

0.0410 

4.91 

0.7718 

« 

0.05 

0.0196 

3-73 

0.3680 

« 

O.IO 

0.0504 

9.82 

0.9486 

« 

O.IO 

0.0133 

7.46 

0.2509 

u 

O.2O 

0.0634 

19.63 

1.1930 

« 

0.20 

0.0087 

14.92 

0.1636 

KHSO4  (20°) 

O.OI 

0-0375 

1.36 

0.706 

KC1O3 

0.025 

0.0256 

3.06 

0.4821 

u 

0-02 

0.0500 

2.72 

0-941 

" 

O.O5 

0.0197 

6.13 

0.3716 

« 

O.IO 

0-1597 

13.62 

3.006 

" 

O.IO 

0.0138 

12.26 

0.2601 

KHC2O4*  (20°)  o.oi 

0.0369 

1.28 

0.694 

" 

O.2O 

0.0092 

24.52 

0.1728 

« 

0.02 

0.0424 

2.56 

0.798 

KBr 

O.O5 

0.0197 

5-95 

0.3699 

« 

O.IO 

0.1132 

12.82 

2.130 

« 

O.IO 

0.0134 

11.91 

0.2517 

HC1 

0.013 

0.0367 

0-45 

0.690 

« 

O.2O 

0.0087 

23.82 

0.1629 

" 

0.025 

0.0428 

0.91 

0.806 

KI 

0.05 

0.0196 

8.30 

0-3687 

« 

0.050 

0.0589 

1.82 

1.109 

« 

O.IO 

0.0132 

16.61 

0.2492 

NaCl 

0.05 

0.0376 

2.92 

0.708 

tt 

O.2O 

0.0086 

33-22 

0.1619 

" 

O.IO 

0.0397 

5-85 

0.748 

KNO3 

O.05 

0.0195 

5.06 

0.3676 

« 

O.2O 

0.0428 

11.70 

0.805 

« 

O.IO 

0.0136 

IO.I2 

0-2551 

NaCIO, 

O.O5 

0.0382 

5-32 

0.718 

« 

O.2O 

0.0090 

20.24 

0.1696 

« 

O.IO 

0.0405 

10.65 

0.763 

K2S04 

0.05 

0.0208 

4-36 

0.3921 

u 

O.2O 

0.0446 

21.30 

0.840 

O.IO 

0.0147 

8.72 

0.2769 

*  Acid  potassium  oxalate. 

« 

O.2O 

O.OIOO 

17.44 

0.1881 

SOLUBILITY  OF  MONO   POTASSIUM  TARTRATE  IN  AQUEOUS  ALCOHOL 

SOLUTIONS. 

(Roelofsen  —  Am.  Ch.  J.  16,  466,  '94;  Wenger  —  Ibid.  14,  624,  '92.) 

NOTE.  —  The  original  results  were  plotted  on  cross-section  paper  and 
the  following  figures  read  from  the  curves. 


o 

10 
20 

25 
30 

40 

50 


Milligrams  KHC4H4O6  per  10  cc.  of  Aq.  Alcohol  of; 


10 

20 

3° 

40 

60 

so 

per  cent. 

per  cent. 

per  cent. 

per  cent. 

per  cent. 

per  cent. 

17 

II 

7 

6 

6 

6 

22 

14 

8 

7 

6 

6 

29 

18 

ii 

8 

6 

6 

34 

21 

12 

9-5 

6-5 

5-5 

40 

25 

13 

ii 

7 

5-5 

55 

36 

19 

14 

7-5 

5 

87 

55 

29 

19 

8 

5 

POTASSIUM    FLUO    TITANATE    K2TiF6.H2O. 
SOLUBILITY  IN  WATER. 

(Marignac  —  Ann.  chim.  phys.  [4]  8,  65,  '66.) 

t°  o°    3°    6°    10°   14°   20° 

Cms.  K2TiF6  per  100  gms.  H2O  0.55  0.67  0.77  O.QI  1.04  1.28 


267  POTASSIUM   VANADATB 

POTASSIUM    VANADATE    K3V5O14.5H2O. 
100  grams  H2O  dissolve  19.2  grains  at  17.5°. 

(Radan  —  Liebig's  Ann.  251,  120,  '89.) 

POTASSIUM    ZINC    VANADATE    KZnV6O14.8H2O. 
100  grams  H2O  dissolve  0.41  gram  of  the  salt  (Radan). 

PRASEODYMIUM    SULPHATE    Pr2(SO4)3. 
SOLUBILITY  IN  WATER. 

(Muthmann  and  Rolig  —  Ber.  31,  1727,  '98.) 


Gms.  Pr2(SO4)3 
t  °.                per  100  Gms. 

Solid 
Phase.              ' 

Gms.  Pr2(SO4)3 
per  loo  Gms. 

Solid 

DU 

Solution. 

Water. 

Solution. 

Water. 

>                .rnase. 

0 

I6.5 

19.8 

Pr2(S04)3.8H20  75 

4-0 

4.2 

Pr2(SO4)3.8H2O 

18 

12-3 

I4-I 

85 

1-5 

J-55 

Pr2(S04)3.8H20  + 

35 

9-4 

IO-4 

" 

Pr2(S04)3.5H20 

55 

6.6 

7-1 

95 

I  .0 

I  .01 

Pr2(S04)3.5H20 

PROPIONIO    ALDEHYDE    C2H5COH. 

100  grams  H2O  dissolve  16  grams  aldehyde  at  20°. 

(Vaubel  — J.  pr.  Ch.  59,  30,  '09.) 

PROPIONITRIL    C2H5CN. 

SOLUBILITY   IN  WATER. 
Synthetic  method  used.     See  Note,  page  9. 

(Rothmund  — Z.  physik.  Ch.  26,  474,  '98.) 

Wt.  per  cent  C2HSCN  in;  Wt.  per  cent  C2H5CN  in: 

*    '  Aq.  C2H5CN  **•  A^  C2H5CN 

Layer.  Layer.  Layer.  Layer. 

40  10.7  92.1  95                 19.6  78.0 

50  ii. 6  90.5  ioo                 22.4  75.5 

60  12.7  88.5  105                   26.0  72.1 

70  13.2  86.1  no                 32.0  66.5 

80  14-9  83.4  113 .1  (crit.  temp.)  48.3 

90  17.6  80.2 

PROPYL    ACETATE,    Butyrate   and    Propionate. 

SOLUBILITY  OF  EACH  IN  AQUEOUS  ALCOHOL  MIXTURES. 

(Bancroft  —  Phys.  Rev.  3,  205,  '95,  calc.  from  Pfeiffer.) 


cc.  H2O  Add 

ed  to  Cause  S< 

JL. 

jparation  *  in  : 

cc.  H2O  Added  to  cause  Separation*  i 

hoi  in           P.  Ace- 
Mixture,          tate. 

P.  Buty- 
rate. 

P.  Propio- 
nate. 

cc.  Alco- 
hol in 
Mixture. 

P.  Ace-      P.Buty- 
tate.           rate. 

P,  Propio- 
nate. 

3 

4-5o 

I.I9 

1.58 

21 

58.71      19.68 

27.83 

6 

10.48 

3-55 

4-70 

24 

00          23.72 

33-75 

9 

17.80 

6.13 

8-35 

30 

32  .10 

47-15 

12 

26  .00 

12.54 

36 

41-55 

63.18 

15 

35-63 

12.31 

17-15 

42 

51  .60 

83-05 

18 

47-50 

15.90 

22.27 

48 

62  .40 

107.46 

54 

73  85 

*  cc.  H2O  added  to  cause  the  separation  of  a  second  phase  in  mixtures  of  the  Riven  amounts  of  alcohol 
and  3  cc.  portions  of  propyl  acetate,  butyrate  and  propionate, 


PROPYL    ACETATE  268 

SOLUBILITY  OF  PROPYL  ACETATE,  FORMATE,  AND  PROPIONATE 

IN  WATER. 

100  cc.  H2O  dissolve  1.7  gms.  propyl  acetate  at  22°. 
100  cc.  H2O  dissolve  2.1  gms.  propyl  formate  at  22°. 

(Traube  —  Her.  17,  2304,  '84.) 

ioo  cc.  H2O  dissolve  0.6  cc.  propyl  propionate  at  25°.  (Bancroft.) 


PROPYL    CHLORIDE,  Bromide,  etc. 

SOLUBILITY  IN  WATER. 

(Rex  — Z.  physik.  Ch.  55,  355,  '06.) 

Grams  P.  Compound  per  ioo  Gms.  H2O  at: 


Propyl  Compound. 


O    .  10    .  20    .  30    . 

CH3CH2CH2C1  (normal)  0.376  0.323  0.272  0.277 

CHgCHLjCKjBr       "  0.298  0.263  0.245  0.247 

CH3CH2CH2I  0.114  0.103  0.107  0.103 

(CH3)2CHC1  (iso)  o .  440  o .  363  o .  305  o .  304 

(CH3)2CHBr    "  0.418  0.365  0.318  0.318 

(CH3)2CHI       "  0.167  0.143  0.140  0.134 


PROPYLENE   C3H6.     SOLUBILITY  IN  WATER. 

(Than  —  Liebig's  Ann.  123,  187,  '62.) 
t°.  ft.  q. 

o      0.4465      0.0834 
5      0.3493      0.06504 
10      0.2796      0.0519 

15         0.2366         0.0437 
2O         O.22O5         0-0405 

For  values  of  (3  and  q,  see  Ethane,  page  133. 


PYRENE  C16H10 

SOLUBILITY  IN  TOLUENE  AND  IN  ABSOLUTE  ALCOHOL. 

ioo  gms.  toluene  dissolve  16.54  gms.  pyrene  at  18°. 
ioo  gms.  absolute  alcohol  dissolve  1.37  gms.  pyrene  at  10°  and  3.08 
gms.  at  b.  pt. 


PYROGALLOL    C6H3(OH)3  i,  2,  3. 

SOLUBILITY  IN 
(u.  s 

ioo  gms.  water  dissolve  62.5  gms.  C6H3(OH)3  at  25°. 


SOLUBILITY  IN  WATER,  ETC. 
(u.  s.  P.) 


ioo  gms.  alcohol  dissolve  100.0  gms.  C6H3(OH)3at  25°. 
ioo  gms.  ether  dissolve  90.9  gms.  C6H3(OH)3  at  25°. 


269 


QUININE 


QUININE    C20H24N2O2.    (See  also  Cinchona  alkaloids,  p.  117.) 

SOLUBILITY  OF  QUININE  AND  OF  QUININE  SALTS  IN  WATER  AND 
OTHER  SOLVENTS. 

(U.  S.  P.) 

Grams.  Quinine  Compound  per  100  Grams  Solvent  in: 
Compound. 

C20H24N202 
C20H24N202.3H20 
C20H24N202HC1.H20 
C20H,4.N202.2C6H4(OH). 

COOH.H2O 

(C20H24N202)2.H2S04.7H20 
C20H24N202.H2S04.7H20 
C20H24N202.HBr.H20 


Water. 

Alcohol. 
At  25°. 
166.6 
166.6 

166.6 

9.09 
1.16 

5-55 
149.2 

Ether.    Chloroform. 
At  25°.         At  25. 
22.2            52.6 
76.9            62.5 
0.417    122.  O 

0.91             2.70 
...                0.25 

0.056      o.  109 

6.2 

Glycerine. 
At  25°. 
0.633 
0.472 
12.  2 

6.25 
2.78 

5-55 
12.5 

At 
0. 
0. 

5- 
i. 

0. 

II. 

2. 

25°- 

057 
065 

55 

30 
i39 

77 
5 

At  80°. 
0.123 

o.  129 

250.0 

2.86 

2.  22 

II7.7 

33-3 

SOLUBILITY  OF  QUININE  IN  AQUEOUS  SOLUTIONS  OF  CAUSTIC  ALKALIES. 

(Doumer  and  Deraux  —  J.  pharm.  chim.  [6]  i,  50,  '95.) 

METHOD.  —  A  one  per  cent  solution  of  quinine  sulphate  containing 
a  very  small  amount  of  HC1  was  gradually  added  to  200  cc.  portions 
of  the  caustic  alkali  solutions  of  the  various  concentrations  stated, 
and  the  point  noted  at  which  a  precipitate  of  the  appearance  cor- 
responding to  that  of  i  cc.  of  milk  in  100  cc.  of  water,  remained 
undissolved. 

In  Aq.  Ammonia.     In  Aq.  Sodium  Hydrate.     In  Aq.  Pot.  Hydrate. 

Gms.KOH    Gms.  Anhydrous 


Gms.NH3 

Gms.  Anhydrous 

per  200  cc. 
Solution. 

Quinine 
Dissolved. 

0.52 

0-084 

0.65 

0.084 

4-59 

0-096 

13.08 

O-I22 

18.88 

0.144 

25.19 

0.174 

35-79 

0.184 

Gms.NaOH 
per  200  cc. 
Solution. 

Gms.  Anhydrous 
Quinine 
Dissolved. 

0.007 

O.O92 

O-OI2 

O.O9I 

0-740 
2  .l6o 
3.188 
6.172 

8-537 

0.090 
0.079 
0-056 
O.O44 
0-021 

17.074 

O.OI5 

per  200  cc. 
Solution. 

0.612 

1.512 
10.944 

44 • 7°4 


Quinine 
Dissolved. 

0.088 
O.O82 
0.068 
0.039 
O.OO6 


Salt. 


Brom  Hydrate  (basic) 
(neutral) 


Chlor  Hydrate  (basic) 


Lactate 
« 


SOLUBILITY  OF  QUININE  SALTS  IN  WATER. 

(Regnault  and  Willejean  —  Chem.  Centralb.  18,  252,  '87.) 

-o       Gms.  Salt  per  <;  u  to 

*    '     iooGms.H20. 

2.06         Salicy late  (basic)    15 
Sulphate     "          14 
16 
18 
"       (neutral)  15 


14 

12 
14 

16 
15 

12 
14 
15 

37 


12-33 

13-19 

14.79 

14.20 

3.80 

4.14 

4-25 
10.03 
16.18 


18 


Gms.  Salt  per 
loo  Gms.  H2O 

O.II4 
0.139 

o .  153 

0.160 

8.50 

8.90 

9.62 


Valerate  (basic)     12-162.59 


RESORGINOL. 


270 


RESORCINOL   C6H4(OH)2  i,  3. 

SOLUBILITY  IN: 
Water.  Ethyl  Alcohol. 

(Speyers  —  Am.  J.  Sci.  [4]  14,  294,  '02.)  (Speyers.) 


O 
10 
20 

25 
30 

40 

50 
60 
70 
80 

NOTE.  —  The  original  results  of  Speyers  are  given  in  terms  of 
mols.  per  ioo  mols.  H2O. 

According  to  Vaubel,  ioo  gms.  H2O  dissolve  175.5  gms-  C6H4(OH)2» 
or  ioo  gms.  sat.  solution  contain  63.7  gms.  at  20°.  Sp.  Gr.  of  sol. 
=  I-I335-  (J.  pr.  Ch.  [2]  52, 73.  '95-) 

SOLUBILITY  OF  RESORCINOL  IN  BENZENE. 

(Rothmund  —  Z.  physik.  Ch.  26,  475,  '98.) 

Synthetic  method  used.     See  Note,  p.  9. 

Gms.  C6H4(OH)2  per  ioo  Gms. 


Sp.Gr.of     C 
Solutions. 

rms.C6H4(OH)2  per  ioo  Gms. 

Water. 

Solution. 

I  .IOI 

60 

37-5 

1.118 

8l 

44.8 

I-I34 

103 

5°  -7 

I  .142 

117 

53-9 

1.148 

56-7 

I-I57 

161 

58.9 

1.165 

198 

66.5 

1.172 

246 

71.1 

i  .176 

320 

76.2 

1.179 

487 

82.9 

Sp.Gr.of     < 
Solutions. 

jms.  CsH4(OH)2  per  ioo  Gms. 

Alcohol. 

Solution. 

1-033 

2IO 

67.8 

1.036 

223 

69.0 

I  .041 

236 

70-3 

1.045 

243 

70.8 

I  .048 

250 

71.4 

I  .056 

266 

72.7 

1.065 

286 

74-1 

I  .075 

311 

75-7 

1.087 

34i 

77-3 

I  .104 

375 

78.9 

C6H6  Layer.  C6H4(OH)2  Layer. 

60  4-8  79.4 

7o  6.6  77.5 

80  9.2  75.0 


0  Gms.  C6H4(OH)2  per  100  Gms. 

C6H6  Layer.     C6H4(OH)2  Layer 
90  13.0  71.3 

ioo  19.5  65.7 

105  24.6  60.7 

109.3  (crft-  temp.)     42.4 


DISTRIBUTION  OF  RESORCINOL  BETWEEN  WATER  AND  ORGANIC 
SOLVENTS  AT  ORDINARY  TEMPERATURE. 

(Vaubel  —  J.  pr.  Ch.  [2]  67,  478,  '03.) 
Gms. 

C6H4(OH)2  Solvents. 

Used. 

i  .191  60  cc.  H2O+  30  cc.  Ether 

i  .191  60  cc.  H2O+  60  cc.  Ether 

0-800  40  cc.  H2O+  40  cc.  Benzene 

0.800  40  cc.  H2O+  80  cc.  Benzene 

0.500  50  cc.  H2O+   50  cc.  CC14 

0.500  50  cc.  H2O+ioo  cc.  CC14 

0.500  50  cc.  H2O+i5o  cc.  CC14 


Gms.  Cfl] 

EI4(OH)  in: 

H2O  Layer. 
0.2014 

Organic 
Solvent  Layer. 

0.9896 

0.2475 
0-5873 

0-9525 
0.2127 

o-5773 

0.4885 
0.4880 
0.4880 

O.2227 
O.OII5 
O-OI2O 
O.OI2O 

RHODIUM    SALTS.     SOLUBILITY  IN  WATER. 

(Jorgensen  —  J.  pr.  Ch.  [2]  27,  433.  '83;  34.  394.  '86;  44,  SL  '91  •) 
Salt.  Formula.  t°. 

Chloro  Purpureo  Rhodium  Chloride  ClRh(NH3)5Cl2  17 

Luteo  Rhodium  Chloride  Rh(NH3)6Cl3  8 

Luteo  Rhodium  Nitrate  Rh(NH3)6(NO3)3  ord.  t. 


Luteo  Rhodium  Sulphate 


[Rh(NH3)6]2(S04)3.5H20      20 


Gms.  per  ioo 

Gms.  H2O 

0.56 

13-3 
2.  I 

2-3 


271                        RUBIDIUM    ALUM 

RUBIDIUM    ALUMS. 

SOLUBILITY  IN  WATER. 

(Locke  —  Am.  Ch.  J.  27,  174,  *oi.) 
Gms.  Alum  oer  ioo  Gms.  H*O. 

p  _  __i 

t  ° 

^ 

Anhydrous. 

Hydrated. 

G.  Mols. 

Rb.  Aluminum  Alum 

RbAl(SO4)2.i2H2O 

25 

1.81 

3-15 

0.0059 

. 

" 

3° 

2.19 

0.0072 

11 

" 

35 

2.66 

0.0087 

11 

" 

40 

3.22 

0.0106 

Rb.  Chromium  Alum 

RbCr(S04)2.i2H20 

25 

2-57 

4-34 

o.  0079 

" 

" 

3° 

.  .  . 

o.  0096 

" 

" 

35 

4-  IJ 

. 

0.0128 

" 

" 

40 

5-97 

. 

0.0181 

Rb.  Vanadium  Alum 
Rb.  Iron  Alum 

RbV(SO4)2.i2H2O 
RbFe(SO4)2.i2H2O 

25 
25 

5-79 
9-74 

9-93 
16.98 

0.0177 
0.0294 

" 

U 

3° 

20.  24 

0.0617 

Biltz  and  Wilke  (Z.  anorg.  Ch.  48,  299,  '06)  find  for  the  solubility  of 
rubidium  iron  alum  in  water,  at  6.6°,  4.55  gms.  per  100  cc.  solution; 
at  25°,  29.0  gms.;  and  at  40°,  52.6  gms. 


RUBIDIUM    FLUOBORIDE    RbBF4. 

100  gms.  H2O  dissolve  0.55  gm.  RbBF4  at  20°,  and  i.o  gram  at  100°. 

(Godeffroy  —  Ber.  9,  1337,  '76.) 

RUBIDIUM    BROMIDE    RbBr. 

SOLUBILITY  IN  WATER. 

(Rimbach  —  Ber.  38,  1557,  '05.) 

Gms.  RbBr  per  ioo  Gms.  Gms.  RbBr  per  TOO  Gms. 

'  Water.  Solution.  Water.  Solution. 

0-5  89.6  47.26  39.7          I3I-85  56.87 

5.0          98.0        49-50  57-5       J52-47        60.39 

16.0        104.8        S1-1?  I][3-5       205.21        67.24 


RUBIDIUM    CARBONATE    Rb2CO3. 

100  gms.  absolute  alcohol  dissolve  0.74  gm.  Rb2CO3. 

(Bunsen.) 

RUBIDIUM    CHLORATE    RbClO3. 

SOLUBILITY  IN  WATER. 

(Reissig  —  Liebig's  Ann.  127,  33,  '63.) 
t°.  4.7°.          13.0°.  18.2°.         19-0°. 

Gms.  RbClO3  per  ioo  grams  H2O         2.8        3.9        4.9        5.1 


RUBIDIUM    (Per)    CHLORATE    RbClO4. 

ioo  grams  H2O  dissolve  1.08  grams  RbClO4  at  21.3°. 

(Longuimine  —  Liebig's  Ann.  121,  123,  '62.) 


RUBIDIUM   CHLORIDE  272 

RUBIDIUM    CHLORIDE    RbCl. 

SOLUBILITY  IN  WATER. 

(Rimbach  —  Ber.  35,  1304,  '02;  Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203  A,  207,  '04.) 
to       Mols.  RbCl    Gms.  RbCl  per  100  Gms.  Mols.  RbCl    Gms.  RbCl  per  100  Gms. 

per  Liter.          Water.          Solution.  per  Liter.          Water.          Solution. 

o  5.17  77.0  43-5  60  6.90  115.5  53.6 

10  5.55  84.4  45.8  70  7.12  121.4  54-8 

20  5.88  91.1  47.7  80  7.33  127.2  56.0 

33  6.17  97.6  49.4  90  7.52  133.1  57.1 

40  6.43  103.5  5°-9  I0°  7-71  J38-9  58-9 

50  6.67  109.3  52-2  112.9  7.95  146.6  59.5 

RUBIDIUM    TELLURIUM    CHLORIDE    Rb2TeCl6. 

100  gms.  Aq.  HC1  of   1.2  Sp.  Gr.  dissolve  0.34  gm.  Rb2TeCl6  at  23°. 
100  gms.  Aq.  HC1  of  1.05  Sp.  Gr.  dissolve  13.09  gms.  Rb2TeCl6  at  23°. 

(Wheeler  — Am.  J.  Sci.  [3]  45,  267,  '93-) 

RUBIDIUM    THALLIUM    CHLORIDE    3RbClTlCl3.2H2O. 
100  gms.  H2O  dissolve  13.3  gms.  at  18°,  and  62.5  gms.  at  100°. 

(Godeffroy  —  Zeit.  allgem.  Oster.  Apoth.  No.  9,  '80.) 

RUBIDIUM    CHROMATE    (Mono)    Rb2CrO4. 
SOLUBILITY  IN  WATER. 

(Schreinemaker  and  Filippo  —  Chem.  Centralb.  77,  I,  1321,  '06.) 


Gms.  RbCrO4 
t°.             per  loo 

Gms.  RbCrO4 
t°.                per  100 

Gms.  RbCrO4 
t  °  .                  per  too 

Gms.  Solution. 

Gms.  Solution. 

Gms.  Solution. 

-  7 

36-65 

50            47-44 

—  2  .40 

I5-58 

o 

38-27 

60  .  4        48  .  90 

—  3  .25 

20.03 

10 

40.23 

Solid  Phase,  Ice 

-4-14 

24.28 

20 

42.42 

—  0.6          6.95 

-5-55 

30-15 

30 

44.11 

—  i.i           7  .22 

-6.71 

34-31 

40 

46-13 

-1.57        9.87 

about  —  7 

36-65 

RUBIDIUM    (Di)    CHROMATE    Rb2Cr2O7. 

zoo  grams  saturated  aqueous  solution  contain  9.47  grams  Rb2Cr2O7 
at  30°. 

(Schreinemaker  and  Filippo.) 

RUBIDIUM    HYDROXIDE    RbOH. 

loo  grams  sat.  aqueous  solution  contain  63.39  grams  RbOH  at  30°. 

(Schreinemaker  and  Filippo.) 

RUBIDIUM    IODATE    RbIO3. 

loo  grams  H2O  dissolve  2.1  grams  RbIO3  at  23°. 

(Wheeler  — Am.  J.  Sci.  [3]  44,  123,  '92.) 

RUBIDIUM    IODIDE    Rbl. 

loo  grams  H2O  dissolve  137.5  grams  Rbl  at  6.9°,  and  152.0  grams  at 

J7-4   •  (Reissig  — Liebig's  Ann.  127,  33.  '63.) 


273  RUBIDIUM   IODIDE 

SOLUBILITY  OF  RUBIDIUM  IODIDE  IN  ORGANIC  SOLVENTS. 

(Walden  — Z.  physik.  Ch.  55,  713,  718,  '06.) 
Solvent.  Formula.  Grams  Rbl  per  TOO  cc.  Solution. 

Acetonitril  CH3CN  1.478  at  o°  1.350  at  25° 

Propionitril  C2H5CN  0.274     "  0-305     " 

Nitromethane  CH3NO2  0.567     "  0.518      " 

Acetone  (CH3)2CO  0.960     "  0.674      " 

Furfurol  C4H3O.COH  4.930      " 

RUBIDIUM    BROM    IODIDE    RbBrJ. 

100  gms.  sat.  aq.  solution   contain   about   44.0   gms.    RbBr2I,   and 
the  Sp.  Gr.  of  the  solution  is  3.84. 

(Wells  and  Wheeler  — Am.  J.  Sci.  [3]  43,  475,  '92.) 

RUBIDIUM    NITRATE    RbNO3.      SOLUBILITY  IN  WATER. 

(Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203  A,  207,  '04.) 


».. 

Mols. 
RbN03    - 
Per  Liter. 

Grams  RbNOs  per  ioo  Gms.       ^  0 

Mols.       C 
RbN03 
Per  Liter. 

1ms.  RbNOs  per  ioo  Gms 

Water. 

Solution. 

Water 

Solution  . 

o 

1.27 

19-5 

I6.3 

60 

7-99 

200 

66.7 

10 

2  .04 

33-o 

24.8 

70 

9.02 

251 

71-5 

20 

3.10 

53-3 

34-6 

80 

9-93 

309 

75-6 

30 

4-34 

81.3 

44.8 

90 

10.77 

375 

78.9 

40 

5.68 

116.7 

53-9 

IOO 

n-54 

452 

81.9 

5° 

6.88 

155-6 

60.9 

118.3 

12  .76 

6l7 

86.1 

RUBIDIUM    PERMANGANATE    RbMnO4. 

One  liter  of  aqueous  solution  contains  6.03  grams  RbMnO4  at  7°. 

(Muthmann  and  Kuntze  —  Z.  Kryst.  Min.  23,  3771  '94.) 

ioo  cc.  sat.  aq.  solution  contain  0.46  gm.  RbMnO4  at  2°,  1.06  gms.  at 

19°  and  4.68  gms.  at  60°.  (Patterson—  J.  Am.  Ch.  Soc.  28,  1735,  '06.) 

RUBIDIUM    SELENATE    Rb2SeO4. 

ioo  grams  H2O  dissolve  158.9  grams  Rb2SeO4  at  12°. 

(Tutton  —  J.  Ch.  Soc.  71,  850,  '97.) 

RUBIDIUM    FLUO    SILICATE    Rb2SiF6. 

ioo  gms.  H2O  dissolve  0.16  gm.  Rb2SiF6  at    o°,  and  1.36  gms.  at  100°. 

(Stolba  —  J.  pr.  Ch.  101,  i,  '67.) 

RUBIDIUM    SILICO    TUNGSTATE    Rb8SiW12O42. 

ioo  gms.  H2O  dissolve  0.65  gm.  Rb8SiW12O42  at  20°,  and  5.1  gms.  at 

I OO°.  (Godeffroy  —  Ber.  9,  1363,  '76.) 

RUBIDIUM    SULPHATE    Rb2SO4.      SOLUBILITY  IN  WATER. 

(Etard  — Ann.  chim.  phys.  [7]  2,  550,  '94;  Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203   A,  207,  '04.) 


t  °. 

Mols.       r 
Rb2S04     <- 
per  Liter. 

rms.  Rb2SO4 

j>er  ioo  Gms 

—      t°. 

Mols.       o 
Rb2SO4     /— 
per  Liter. 

ms.  Rb2SO4  per  ioo  Gms. 

Water. 

Solution. 

Water. 

Solution. 

o 

1.27 

36-4 

27-3 

60 

2-15 

67.4 

40-3 

10 

I  .46 

42  .6 

29.9 

70 

2.25 

71.4 

41-7 

20 

I  .64 

48.2 

32-5 

80 

2-34 

75-o 

42-9 

30 

1-79 

53-5 

34-9 

90 

2.42 

78.7 

44.0 

40 

I  .92 

58.5 

36-9 

IOO 

2.49 

81.8 

45-o 

50 

2.04 

63.1 

38-7 

102.4 

2.50 

82.6 

45-2 

RUBIDIUM    SULPHATE  274 

SOLUBILITY  OF  RUBIDIUM  DOUBLE  SULPHATES  IN  WATER  AT  25°. 

(Locke  —  Am.  Ch.  J.  27,  459,  '01.) 

Per  IPO  cc.  H2O.  Per  100  cc.  H2O. 

Formula.                   Cms.           Mols.  "                        Formula.  Cms.      '     Mols.   ' 

Anh.  Salt.       Salt.  Anh.  Salt.       Salt. 

Rb2Cd(SO4)2.6H2O      76.7      0.1615          Rb2Mn(SO4)2.6H2O  35.7      0.0857 

Rb2Co(SO4)2.6H2O        9.28    0.022            Rb2Mg(SO4)2.6H2O  20.2      0.0521 

Rb2Cu(SO4)2.6H2O       10.28    0.0241           Rb2Ni(SO4)2.6H2O  5.98    0.0142 

Rb2Fe(SO4)2.6H2O       24.28    0.0579          Rb2Zn(SO4)2.6H2O  10.10    0.0236 

SALICYLIC    ACID    C6H4.OH.COOH  i  :2. 

SOLUBILITY  IN  WATER.     (See  also  p.  61.) 


Ibid.  27,  315,  '98;  Hoffmann  and  Langbeck  —  Ibid.  51,  400,  '05.  For  determinations  not  in  good  agreement 
with  the  following,  see  Alexejew  —  Ann.  Physik.  Chem.  28,  305,  '86;  Bourgion  —  Ann.  chim.  phys.  [5] 
iSs  165,  '78;  Ost.—  J.  pr.  Ch.  [2]  17,  232,  '78.) 


Gms. 
ho        CeH^OHCOOH 
per 

Gms. 
to         C6H4OH.COOH 
per 

Gms. 
fc0          C6H4OH.COOH 
oer 

Liter  Solution. 

Liter  Solution. 

Liter  Solution. 

0 

0.8 

25 

2  .2 

60 

8.2 

10 

I  .2 

3° 

2-7 

70 

I3.2 

20 

1.8 

40 

3-7 

80 

20-5 

5o 

5-4 

SOLUBILITY  OF  SALICYLIC  ACID   (LIQUID)  IN  WATER. 

(Alexejew.) 

Determinations  by  Synthetic  Method.     See  Note,  page  9.     Figures 
read  from  curve. 

Gms.  C0H4OHCOOH 
per  100  Gms. 

t°.  Aqueous  Salicylic  Acid 

Layer.  Layer. 

60         7         68 
70          8          64 

80  12  58 

90         19          49 
95  (crit.  temp.)     32 

SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SALT  SOLUTIONS  AT  25° 

AND   AT  35°. 
(Hoffmann  and  Langbeck  —  Z.  physik.  Ch.  51,  407,  '05.) 

Normalit 
Salt. 


KC1 

tt 


KN03 

a 

it 
tt 

NaCl 

a 

u 
It 


Normality 
of  Salt 

Gms. 
Salt  per 

V^fVL-L^Vyi-lV-V/W  11                                                         * 

dissolved  at  25°. 

dissolved'  at  35°. 

Solution. 

Liter. 

Gms.  per  1000  G.  Molecular  Gms.  p 

er  1000 

G.  Molecular 

gms.  Sat.  Sol. 

percentage,      gms.  S 

iat.  Sol. 

percentage. 

0.0 

O.O 

2 

.206 

2 

•8851 

3 

.197 

O.O2O 

1.49 

2 

.24 

2 

.9216. 

io~4 

3 

•23 

4 

.22o6.I< 

_- 

o.ioo 

7.46 

2 

•25 

2 

•9377 

it 

3 

•23 

4 

.2203 

" 

0.492 

36.73 

2 

.02 

2 

.6321 

a 

3 

.01 

3 

.9268 

a 

1  .004 

74-92 

I 

.89 

2 

•4759 

tt 

2 

.68 

3 

•5003 

tt 

O.02O 

2  .02 

2 

•25 

3 

•9351 

tt 

3 

•25 

4 

•2499 

it 

o  .100 

IO-I2 

2 

•30 

3 

•0103 

it 

3 

•32 

4 

•3334 

" 

0.504 

51.10 

2 

•38 

3 

.1061 

a 

3 

•38 

4 

.4123 

it 

I  .004 

101  .60 

2 

•39 

3 

.1249 

n 

3 

•36 

4 

•3848 

tt 

O.020 

I.I9 

2 

•23 

2 

.9110 

tt 

3 

.22 

4 

.2062 

it 

O.IOO 

5-95 

2 

.22 

2 

.9027 

tt 

3 

.20 

4 

.1806 

tt 

0-497 

29.50 

2 

•  OO 

2 

.6128 

tt 

2 

•85 

3 

.7171 

" 

0.988 

58.80 

I 

.72 

2 

.2487 

n 

2 

•43 

3 

.1596 

" 

275 


SALICYLIC    ACID 


SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
FORMATE,  ACETATE,  AND  BUTYRATE  AT  26.4°. 

(Philip  — J.  Ch.  Soc.  87,  992,  '05.) 

Mols-Na  SaIt^^C6H4.OH.COOH  per  Liter  in:        Cms    Na     Cms.  Ce^OHCOOH  per  Liter  in: 
ioo 
perLiter- 


ioo     -    - 

HCOONa.  CH3COONa.  C 

I.7I               1.71 

1.71 

2-35           2.47 
3-05          3-35 

2.50 
3-48 

3-7             4-2 

4-35 

4-3            5-1 
4.8            6.1 

5-3 
6-3 

'HCOONa.  CH3COONa.  C3H7COONa 
2.36  2.36  2.36 

3-7  3-6 

5-o  5-2 

6.2  6.75 

7-2  8.3 


3-3 

45 

5-65 

6.85 

8.1 


SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  SODIUM 
SALICYLATE  AT  20.1°. 

(Hoitsema  —  Z.  physik.  Ch.  27,  315,  '98.) 


Solid 
Phase. 

C^OHCOOH 


Gram  Mols 

.  per  Liter. 

Sp.  Gr. 

Grams 

per  Liter. 

C6H4OH 
COOH. 

C6H4OH 
COONa. 

of 
Solutions. 

C6H4OH 
COOH. 

CeH4OH 
COONa. 

0.0132 

O   0 

I  .OO2 

1.823 

O-O 

O-OII2 

0.017 

1.003 

i-55 

2.705 

0-0124 

O.II3 

I  .009 

1.71 

17.98 

0-0143 

0.226 

I  .Ol6 

1.97 

35-96 

O.Ol64 

0-344 

I  .024 

2  .26 

54-74 

O.O2O3 

0.500 

I  .034 

2.80 

79  -56 

0.062 

1.70 

1.098 

8.56 

270.5 

0-095 

2  .11 

I-I37 

13.11 

335-7  { 

0.091 

2  .19 

I.I44 

12-56 

348-4 

0.086 

3-41 

I  .215 

11.88 

542.6 

O.oSl 

4-23 

1.263 

ii  .19 

673  -o{C 

O.O48 

4-l8J 

1.259 

6.63 

665.1 

O-02I 

4-12 

1.258 

2  .90 

665-5 

O-OO 

4-15 

1-257 

O-O 

660.3 

( C6H4OHCOOH.C6H4OHCOONa 

+  C6H4OHCOOH 
C6H4OHCOOH.C6H4OHCOONa 


C6H4OHCOOH.C6H4OHCOONa 
+  C6H4OHCOONa 

Ce^QHCOONa 


SOLUBILITY  OF  SALICYLIC  ACID  IN  ALCOHOLS  IN  ETHER  AND  IN 

ACETONE. 

(Timofeiew  —  Compt.  rend.  112.    1137,  '91;  at  15°.  Bourgoin  — Ann.  chim.  phys.  [5]  13,  405,  '?8; 
at  17°  and  23°,  Walker  and  Wood  —  J.  Ch.  Soc.  73,  620,  '98.) 


Solvent. 

t  °. 

Gms.  C«H4OHCOOH 
per  ioo  Gms. 

Solvent. 

Gms.  CCR.OHCOOH 

t  °_          per  ioo  Gms. 

Solvent. 

Solution. 

Solvent.      Solution. 

CH3OH 

-3 

40. 

67 

28. 

91 

C3H7OH(«) 

~3 

26 

.  12 

20 

•7i 

CH3OH 

+  21 

62. 

48 

38. 

46 

C3H7OH(«) 

+  21 

37- 

69 

27. 

36 

C2H5OH 

~3 

36. 

12 

26. 

29 

(CH3)20 

15 

5°- 

47 

33 

•55 

C2H5OH 

63 

33- 

17 

(CH,)20 

17 

23 

•4* 

C2H5OH 

21 

53- 

53 

34.87 

(CH3)2CO 

23 

31 

3* 

C,H,OH  90% 

IS 

42. 

09 

29. 

62 

*  Per 

ioo  cc.  Sat 

.  Solution. 

SALICYLIC   ACID  276 

SOLUBILITY  OF  SALICYLIC  ACID  IN  AQUEOUS  SOLUTIONS  OF  ETHYL 
ALCOHOL,  .Iso  BUTYL  ALCOHOL,  DEXTROSE,  CANE  SUGAR,  AND  OF 
LEVULOSE  AT  25°  AND  AT  35°. 


Aq.  Solvent. 

H2O 


C4H9OH  (iso) 
« 

« 
« 

C6H1206 


C6.H1206 


(Hoffmann  and  Langbeck  —  Z.  physik.  Ch.  51,  400,  '05.) 

CaH4OHCOOH  dis-              C«H4OHCOOH  dis- 
Conc.  of  Solvent.                        solved  at  25°.                         solved  at  35°. 

Normality. 
O.O 

Gms.  per 
Liter. 

O.O 

Grams                  Grams           Grams 
molecular        per  ioo   gms.  molecular 
percentage.       sat.  solution,  percentage. 

2.8851                 0.22064.1844 

Grams 
per  ioo  gms. 
sat.  solution. 

0.3197 

O. 

0249 

I. 

146 

2.8966.10"^ 

1   o. 

222 

4- 

2044.  io~4 

0.322 

0. 

0560 

2. 

578 

2.9150      " 

0. 

223 

4- 

2348 

tt 

0 

.324 

o. 

1747 

8. 

04 

2.9901 

o. 

229 

0. 

2399 

II. 

05 

4- 

434i 

1C 

O 

.339 

I. 

03 

47- 

4 

3.5279      " 

0. 

270 

5- 

2816 

tt 

0 

.404 

I. 

638 

75-44 

3.9253 

0. 

300 

0. 

020 

i. 

496 

2.909 

0. 

223 

4- 

229 

11 

0 

.324 

o. 

051 

3- 

74 

2-955      " 

o. 

226 

4- 

289 

(I 

0 

•  329 

0. 

IOO 

7.48 

3-033   ;; 

0. 

232 

4- 

435 

11 

0 

•339 

o. 

521 

38. 

60 

o. 

285 

5- 

624 

It 

0-431 

0. 

02 

3-6 

2.886      " 

0. 

221 

4- 

184 

tt 

o 

.321 

0. 

10 

18. 

o 

2.898      " 

0. 

222 

4- 

202 

(I 

0 

.322 

0. 

5° 

89- 

6 

2-954      " 

o. 

226 

4- 

263 

It 

o 

.326 

I. 

00 

180. 

0 

3-OI5 

0. 

231 

4- 

360 

11 

0 

•334 

o. 

02 

6. 

88 

2.885      " 

o. 

221 

4- 

206 

(I 

0 

•322 

0. 

10 

34- 

97 

2.964      " 

0. 

227 

4- 

287 

11 

0 

.328 

0. 

5° 

172. 

o 

3-239 

0. 

248 

4- 

697 

tt 

0 

.360 

I. 

10 

376. 

3 

3-633      " 

o, 

278 

5- 

236 

tt 

0 

.401 

0. 

02 

3- 

6 

2.888      " 

0. 

221 

0. 

06 

10. 

8 

2.895       " 

o. 

221 

0. 

25 

45- 

0 

2.944 

c. 

225 

SOLUBILITY  OF  SALICYLIC  ACID  IN  BENZENE. 

(Walker  and  Wood  — J.  Ch.  Soc.  73»  620,  '98.) 

Gms.                                                     •  Gms.  Gms. 

Ce^OHCOOH                     to            CeH4OHCOOH                to  C^OHCOOH 

per  ioo  Gms.                                           per  ioo  Gms.  per  ioo  Gms. 

CeHs-                                                       CeHg.  CeHe- 


11-7  0.460  30.5  0.991  49.4  2.380 

18.2  °-579  34-6  1.261  64.2  4-40 

36.6  1.430 


SELENIUM    Se. 

SOLUBILITY  IN  CARBON  BISULPHIDE. 

(Marc  —  Z.  anorg.  Ch.  48,  425,  '06.) 

ioo  cc.  CS2  dissolve  0.065  gm-  amorphous  Se  at  room  temperature. 
Se  which  is  heated  to  180°  for  6-7  hours  is  insoluble  in  CS2.  Se  crystal- 
lized from  the  melt  at  200°  is  insoluble  in  CS2.  Se  heated  once  quickly 
to  140°  is  very  slightly  soluble  in  CS2. 

ioo  gms.  methylene  iodide  (CH2I2)  dissolve  1.3  gms.  Se  at  12°. 

(Retgers  —  Z.  anorg.  Ch.  3,  346,  '93.) 


277  SELENIOUS    ACID 


SELENIOUS    ACID    H2SeO3. 

SOLUBILITY  IN  WATER. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  551,  '94.) 


t  o        Cms.  H2SeO3  per 
100  Gms.  Solution. 

t  o        Gms.  H2SeO3  per 
100  Gms.  Solution 

t  o       Gms.  H2SeO3  per 
*     loo  Gms.  Solution. 

—  10 

42.2 

25 

67.0 

60 

79-3 

0 

47-4 

30 

70.2 

70 

79-3 

+  10 

55-o 

40 

77-5 

80 

79-3 

20 

62.5 

5° 

79.2 

90 

79-4 

SILICON    Si. 

SOLUBILITY  IN  LEAD  AND  IN  ZINC. 

(Moissan  and  Siemens  —  Ber.  37,  2088,  '04.) 

In  Lead.  In  Zinc. 

,  o             Gms.  Si  per  100  t  o  Gms.  Si  per  too 

Gms.  Solution.  Gms.  Solution. 

1250            0-024  600  0.06 

1330        0.070  650  0.15 

1400        0.150  730  0-57 

I45O        O-2IO  8OO  0.92 

1550        0.780  850  1.62 


SILICON    IODIDES    Si2I6,    SiI4. 

SOLUBILITY  IN  CARBON  BISULPHIDE. 

(Friedel  and  Lachburg  —  Bull.  soc.  chim.  [2]  12,  92,  '69;  Friedel  —  Liebig's   Ann.  149,  96,  '69) 

ioo  gms.  CS2  dissolve  19  gms.  Si2I6  at  19°. 
100  gms.  CS2  dissolve  26  gms.  Si2I6  at  27°. 
ioo  gms.  CS2  dissolve  2.2  gms.  SiI4  at  27°. 


SILICO    TUNGSTIC    ACID    H8SiW12O42. 

ioo  gms.  H2O  dissolve  961.5  crystallized  silico  tungstic  acid  at  18°, 
and  solution  has  Sp.  Gr.  2.843. 


SILVER  278 

For  equilibrium  between  metallic  Silver  and  mercury  (Silver  amal 
gam)  and  mixed  aqueous  solutions  of  their  nitrates,  determined  foe 
mixtures  of  the  two  metals  in  all  proportions,  see  Reinders  —  Z.  physik. 
Ch.  54,  609,  '06. 

SILVER    ACETATE   CH3COOAg. 

SOLUBILITY  IN  WATER. 

(Nernst  —  Z.  physik.  Ch.  4,379/89;  Arrhenius  —  Ibid,  n,  396,  '93;  Goldschmidt  —  Ibid.  25,  93,  '98, 
Nauman  and  Rucker  —  Ber.  38,  2293,  '05;  Raupenstrauch  —  Monatsh.  Ch.  6,  585,  '85;  Wright  and 
Thompson  —  Phil.  Mag.  [5]  I7t  288,  '84;  19,  i,  '85.) 

to       Gms.Ag(C2H3O2) 
per  Liter. 

o  7.22 

10  8.75 

15  9-4 

20  10.4 

SOLUBILITY  OF  SILVER  ACETATE  IN  AQUEOUS  SOLUTIONS  OF: 
Silver  Nitrate.  Sodium  Acetate. 


to       Gms.Ag(C2H3O2) 
per  Liter. 

t°. 

Cms.  Ag(C2H3O2) 
per  Liter. 

25               II.  2 

50 

16.4 

30               12.  I 

60 

18.9 

40               I4.I 

70 

21.8 

80 

25.2 

AgNOa 

per  Liter. 

Gms.  CH3COOAg  per  Liter  at: 

Gms. 
CHgCOONa 
per  Liter. 

Gms.CHsCOOHg  per  Liter  at: 

16°  (Nernst). 

1  9  .8°  (Arrhenius)  . 

1  6°  (N.,N.andR.). 

i8.6°(A.). 

O 

10.05 

9-85 

O 

10.05 

9.9 

5 

8.2 

7-9 

5 

6-3 

6.6 

10 

7-o 

6.6 

10 

4.6 

4-9 

15 

6.4 

5-5 

15 

3-8 

4.1 

2O 

5-7 

4-5 

20 

3-3 

3-5 

30 

4-4 

30 

2.8 

40 

3-2 

40 

2.4 

SILVER   Mono   Chlor   ACETATE   CH2ClCOOAg. 

One  liter  aqueous  solution  contains  12.97  grams  CH2ClCOOAg  at 

16.9°.  (Arrhenius.) 

SOLUBILITY  OF  SILVER   MONO  CHLOR  ACETATE  AT   16.9°   IN 
AQUEOUS    SOLUTIONS    OF: 

Silver  Nitrate.  Sodium  Chlor  Acetate. 


Gms. 

Gms. 

Gms. 

Gms. 

AgNOs 
per  Liter. 

CH2ClCOOAg 
per  Liter. 

CH2ClCOONa 
per  Liter. 

CH2ClCOOAg 
per  Liter. 

O-O 

12.97 

o.o 

12.97 

9.6 

IO.O5 

3.88 

10.05 

17.0 

7-55 

7-77 

8.16 

15-53 

6.  02 

31.07 

4.19 

58.26 

3-26 

SILVER   Di    Propyl    ACETATE   AgC8H16O2. 

TOO  gms.  H2O  dissolve  0.123  gm.  AgC8H15O2  at  11.7°,  and  0.190  gm. 
at  72°. 

(Furth  —  Monatsh.  Ch.  g,  311,  '88.) 


279  SILVER  ACETATES 

SILVER  Methyl  Ethyl  ACETATE  Ag.CH3.CH2.CH(CH3)COO. 
SILVER  Di  Ethyl  ACETATE  Ag.[(C2H5)2CH.COOJ. 

SILVER  Tri  Methyl  ACETATE  Ag.(CH3)3CCOO.* 
SOLUBILITY  OF  EACH  WATER. 

(Sedlitzky  —  Monatsh.  Ch.  8,  563,  '87;  Keppish  —  Ibid.  9,  589,  '88;  Stiassny  —  Ibid.  12,  601,  '91.) 
Gms.  per  100  Gms.  H2O.  Gms.  per  100  Gms.  H2O. 


I    . 

Ag.C5H9O2. 

AgC6Hu02. 

AgC6H902* 

i    . 

AgC6H902. 

AgC6HnO2. 

AgC6H902* 

0 

I  .112 

0.402 

I  .10 

50 

I  .602 

0-536 

1.47 

10 

I  .126 

0.413 

I  .15 

60 

1.827 

0.585 

20 

I.I82 

0.432 

I  .22 

70 

2.093 

0.643 

1.68 

30 

1.280 

0.458 

I  .22 

80 

2.402 

1.  80 

40 

I  .420 

0-494 

i-37 

SILVER    BENZOATE    C(iH6COOAg. 

One  liter  of  aqueous  solution  contains  1.763  gms.  C6H5COOAg  at 
14.5°,  and  2.607  gms.  at  25°. 

(Holleman  —  Z.  physik.  Ch.  12,  129,  '93;  Noyes  and  Schwartz  —  Ibid.  27,  287,  '98.) 

SOLUBILITY  OF  SILVER  BENZOATE  AT  25°  IN  AQUEOUS  SOLUTIONS  OF: 
Nitric  Acid  (N.  and  S.).  Chlor  Acetic  Acid  (N.  and  S.). 

Millimols  per  Liter.  Grams  per  Liter.  Millimols  per  Liter.  Grams  per  Liter. 


HNO3. 
0.0 
0.004435 
0-00887 
0-00892 
0.01774 
0-02674 

C6H5 
COOAg. 

O.OII44 
0.01395 
0.01698 
0.01715 
0.02324 
0.03071 

HNO3. 
O-O 
0.28o 

o-559 
0.562 
1.118 
1.686 

C6H5 
COOAg. 

2  .607 

3-J95 
3.889 

3.926 

5-321 
7.031 

CH2 
C1COOH. 

o.o 

0.00394 
0-00787 
0.01574 

C6H5 
COOAg. 

O.OII44 
0.01385 

o  01612 

0.02093 

CH2 
C1COOH. 

o.o 

0-371 
0.744 
1.487 

C6H5 
COOAg. 

2.607 
3.172 
3.691 
4.792 

One  liter  of  cold  alcohol  dissolves  0.169  gm.  C6H5COOAg;  one  liter 

Of  boiling  alcohol  dissolves  0.465   gram.  (Liebermann  —  Ber.  35,  1094,  '02.) 

SILVER    BORATE   AgBO2. 

One  liter  of  aqueous  solution  contains  about  9.05  gms.  AgBO2at  25°. 

(Abegg  and  Cox  —  Z.  physik.  Ch.  46,  n,  '03.) 

SILVER    BROMATE    AgBrO3. 

SOLUBILITY  IN  WATER. 

t°.  Gms.  AgBrO3  per  Liter.  Authority. 

2Q  I  .586  (Bottger  — Z.  physik.  01.46,  602,  '03.) 

24.5  1.911  (Noyes  —  Z.  physik.  Ch.  6,  246,  '90.) 

25  I  .  68  (Longi  —  Gazz.  chim.  ital.  13,  87,  '83.) 

SOLUBILITY  OF  SILVER  BROMATE  IN  AQUEOUS  AMMONIA  AND  NITRIC 
ACID  SOLUTIONS  AT  25°. 

(Longi.) 

Grams  AgBrOa  per 

1000  cc.  Sol.         1000  Gms.  Sol. 

Ammonia  Sp.  Gr.  0.998=5%  35.10  35.54 

Ammonia  Sp.  Gr.  0.96  =10%        443-6  462.5 

Nitric  Acid        Sp.  Gr.  i  .21  =35%  3.81  3.12 


SILVER    BROMATE  280 

SOLUBILITY  OF  SILVER  BROMATE  AT  24.5°  IN  AQUEOUS 
SOLUTIONS  OF: 

Silver  Nitrate  (Noyes).  Potassium  Bromate  (N.). 

Normal  Content.  Gms.  per  Liter.  Normal  Content.  Gms.  per  Liter. 


AgN03. 

AgBrO3. 

AgN03- 

AgBrO3. 

KBrO3. 

AgBrO3. 

KBrOs. 

AgBrOa. 

O-O 

o 

,0o8l 

o 

.0 

I  .911 

O 

.0 

O 

.0081 

O-O 

I.QII 

0-0085 

o 

.0051 

I 

•445 

1.203 

o 

.0085 

0 

.00519 

1.42 

1.225 

0.0346 

o 

.0022 

5 

.882 

0.510 

o 

.0346 

0 

.00227 

5-78 

O-SS^ 

SILVER    BROMIDE   AgBr. 

SOLUBILITY  .IN  WATER. 

t  °.  Gms.  AgBr  per  Liter.  Authority. 

2O  O  .000084  (Bottger —  Z.  physik.  Ch.  46,  602,  '03.) 

25  O  .OOOI37  (Abegg  and  Cox  —  Z.  physik.  Ch.  46,  n,  '03.) 

IOO  O.OO37O  (Bottger  — Z.  physik.  Ch.  56,  93,  '06.) 

(See  alsoHolleman  —  Z.  physik.  Ch.  12,  129,  '93;  Kohlrausch  —  Ibid.  50,  365,  '05.) 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  AMMONIA  SOLUTIONS. 

(Longi  —  Gazz.  chim.  ital.  13,  87,  '83;  at  80°,  Pohl  —  Sitzber.  Akad.  Wiss.  Wien,  41,  267,  '60.) 

Gms.  AgBr  at  12°  per  Gms.  AgBr  at  8oo  ^ 

Solvent.  I000  cc.  Iooo  Gms.  *°°°  Gms. 

Solvent.  Solvent.  Solvent. 

Ammonia  Sp.  Gr.  0.998  =  5%      0.114          0.114 

Ammonia  Sp.  Gr.  0.96  =10%     3  -33-4.0    3-47 

Ammonia  Sp.  Gr.  o . 986  ...  ...  0.51*  i.ot 

*  Dried  AgBr.  t  Freshly  pptd. 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF: 

Ammonia  at  o°.  Mono  Methyl  Amine  at  11.5°. 

(Jarry  — Ann.  chim.  phys.  [7]  i?»  363.  '99-)  (Jarry.) 

Grams  per  100  cc.  Solution.  Gms.  per  100  cc.  Solution. 

, » ^  t * N 

NHs  Gas.          AgBr.  NH3  Gas.  AgBr.  NH2CH3.         AgBr. 

3.07    0.080    26.27    1.067       ii. oi    0-07 

4-88  0.096  3I-26  I-568  I3-I7  0.12 

6.69  0.172  33 .89  1.987  15.13  0.16 

8.29  0.212  36-52  2.669  J]C7-97  0.28 

11.51  0.349  37-22  2.888  32.58  0.55 

I5-32  0.557  37-70  2.930  35.62  0.73 

18.09  0.722  39-26  2.892  43-n  1-27 

J9-53  o-74i  39-95  2.852  48-44  2.89 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  THIO  SULPHATE  AT  35°. 

(Richards  and  Faber  —  Am.  Ch.  J.  21,  186,  '99.) 

Gms.  Cryst.  Na  Thio  Sulphate          Gms.  AgBr  Dissolved  Mols.  AgBr  Dissolved 

per  Liter.  per  Gram  of  Thio  Sulphate.       per  Mol.  of 

loo  0.376  0-496 

200  0.390  0.515 

300  0-397  0-524 

400  0-427  0.564 


28i  SILVER    BROMIDE 

SOLUBILITY  OF  SILVER  BROMIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Valenta  —  Monatsh.  Ch.  15,  250,  '94;  see  also  Cohn  — Z.  physik.  Ch.  18,  61,  '95.) 

Gms.AgBr  per  100  Cms.  Aq.  Solution  of  Concentration: 

Salt  Solution.  t°.       , x 

1:100.         5:100.         10:  100.       15:100.       20:100. 

Sodium  Thio  Sulphate  20  0.35       1.90  3.50       4.20       5.80 

"  Calc.  by  Cohn  20  0.50       2.40  4.59       6.58      8.40 

Sodium  Sulphite  25        0.04        ...        0.08 

Potassium  Cyanide  25        ...        6.55        

"  Calc.  by  Cohn  25        ...        6.85        

Potassium  Sulphocyanide          25        ...          ...  o .  73 

Ammonium  Sulphocyanide        20        ...        0.21  2.04       5.30 

Calcium  Sulphocyanide  25        ...          ...  0.53 

Barium  Sulphocyanide  25         ...          .  ..  0.35 

Aluminum  Sulphocyanide          25        ...          ...  4.50 

Thio  Carbamide  25 i  .87        

Thio  Cyanime  25  0.08      0.35  0.72 

NOTE.  —  Cohn  shows  that  the  lower  results  obtained  by  Valenta 
are  due  to  the  excess  of  solid  AgBr  used  and  the  consequent  formation 
of  the  less  soluble  di  salt  3(AgS2O3Na)2  instead  of  the  more  soluble 
salt  (AgS2O3Na)2Na2S203. 

100  cc.  H2O  containing  10  per  cent  of  normal  mercuric  acetate, 
Hg(C2H3O2)2  +  Aq.,  dissolve  0.0122  gram  AgBr  at  20°. 

100  gms.  NaCl  in  cone.  aq.  solution  dissolve  0.474  gm.  AgBr  at  15°. 

100  gms.  NaCl  in  21  per  cent  solution  dissolve  0.182  gm.  AgBr  at  15°. 

100  gms.  KBr  in  cone,  solution  dissolve  3.019  gms.  AgBr  at  15°. 
95  gms.  NaCl  -f  10  gms.  KBr  in  cone.  aq.  solution  dissolve  0.075 
gm.  AgBr  at  15°. 

(Schierholz  —  Sitzber.  K.  Akad.  Wiss.  (Vienna)  101,  2b,  4,  '90-) 


SILVER    BUTYRATE    C3H7COOAg. 


SILVER    (Iso)    BUTYRATE    (CH3)2CHCOOAg. 


SOLUBILITY  OF  EACH  IN  WATER. 

Ch.  25,  93,  '98;  Arrhenius  —  Ibid.  11,  396,  '93;  R 
Ch.  6,  589,  '85-) 

Gms.  per  100  Grams  H2O.  Grams  per  100  Gms.  H2O. 


(Goldschmidt  —  Z.  physik.  Ch.  25,  93,  '98;  Arrhenius  —  Ibid,  n,  396,  '93;  Raupenstrauch  —  Monatsh 

Ch.  6,  589,  '85-) 


Butyrate.            Iso  Butyrate.  Butyrate.  Iso  Butyrate. 

o  0.363  0.796  30  0.561(1.1020.)  i. 060 

10  0.419  0.874  40  0.647  . 

17.8  0.432  (A.)       ...  50  0.742  i-3I3 

18.8  0.445  (A.)  60  0.848 

20  0.484(0.9990.)  0.961  70  0.901  1.670 

25   ...  (1.0440.)  ...  80  1. 14  1-898 


SILVER    BUTYRATE 


282 


SOLUBILITY  OF  SILVER  BUTYRATE  IN  AQ.  SOLUTIONS  OF  SILVER 
ACETATE,  SILVER  NITRATE  AND  OF  SODIUM  BUTYRATE. 

(Arrhenius  —  Z.  physik.  Ch.  n,  396,  '93.) 


In  Silver  Acetate  at  17.8°. 

G.  Mols.  per  Liter.  Grams  per  Liter. 


CH3 
COOAg. 

C3H7 
COOAg. 

CH3 
COOAg. 

C3H7 
COOAg. 

o.o 

0-0221 

o.o 

4-32 

O.O27O 
0-0506 

0.0139 
O.OIO3 

4-51 
8-45 

2.71 
2-01 

In  Silver  Nitrate  at  18.8°. 

G.  Mols.  per  Liter.  Grams  per  Liter. 

C3H. 
COO 


AgNO3. 


C3H7 
COOAg. 


o.o          0.0228 

0.0667      0-0078 

o.ioo       0.0062 


In  Sodium  Butyrate  at  18.2°. 


Ag. 

o.o      4.445 

n-33     1-521 
17.00     1.209 


G.  Mols.  per  Liter.  Grams  per  Liter.  G.  Mols.  per  Liter.  Grams  per  Liter. 


'  CsH7 
COONa. 

o.o 

O.OO66 
0-0164 
0-0329 

C3H7 
COOAg. 

O.O224 
O.OI99 
0.0169 
O.OI3I 

C3H7 
COONa. 

o.o 

o-73 
1.81 

3-62 

COOAg. 

4-363 

3.881 

3.296 

2-555 

C3H7 
COONa. 

0.0658 

0-I3I5 
0.263 

0-493 

C3H7 
COOAg. 

O.OO9I 

o  .  0060 
o  .  0040 

0.0027 

'   C3H7 
COONa. 

7-24 
14-47 
28.96 
54-28 

C3H7 
COOAg. 

i-774 
1.170 
0.780 
0.526 

SILVER    CAPROATES  Ag(C6HuO2). 

SOLUBILITY  IN  WATER. 

(Keppish  —  Monatsh.  Ch.  9,  589,  '88;  Stiassny  —  Ibid.  12,  596,  '91;  Kulisch  —  Ibid.  14,  570,  '93;  Konig 
—  Ibid.  15,  26,  '94;  Altschul  —  Ibid.  17,  568,  '96.) 

Results  in  terms  of  grams  salt  per  100  grams  H2O. 


Methyl  3  Pentan      4  Methyl  Pentan 

Acid  4  4  Acid 

CH3.CH2  CH3(CH2)2CH(CH3) 

:H3CH2COOAg.       .COOAg. 

O  . 076  (A.)     O  . 078(Keppisch)   o  •  l68  (Konig)     o  . 880  (Kulish)    0.510  (Stiassny) 


Normal  Caproate 
I2)4COOAg. 


CHg(CH2 


2  Methyl  Pentan 

4  Acid 

CH3.CH.CH3 
.(CH2)2COOAg.  .CHCH 


O 

0.076  (A.) 

0.078 

10 

0.085 

0.089 

20 

O-IOO 

0-107 

30 

0.123 

0.131 

40 

0.154 

0.161 

50 

0.193 

0.198 

60 

0.240 

0.243 

70 

0.295 

0.288 

80 

o-354 

90 


0.162 

0.163 

0.170 

0.183 
0.203 

0.229 

0.263 
0.300 
0-347 


0.858 
0.849 
0.854 
0.871 
0.902 
0.946 
1.003 
1.073 


0.528 

o-55o 
o-574 
0.602 
0.632 
0.666 
0.702 
0.742 


SILVER    CARBONATE    Ag2CO3. 

SOLUBILITY  IN  WATER. 

t°.      Gms.  Ag2CO3  per  Liter.  Authority. 

15                 0 .031  (Kremers  —  Pogg.  Ann.  85,  248,  '52.) 
25                 O  -033  (0.00012  gm.  atoms  Ag.)     (Abegg  and  Cox  —  Z.  physik.  Ch.  46,  n,  '03.) 

IOO                 0 .50  (Joulin  —  Ann.  chim.  phys.  [4]  30,  260,  '73.) 

J5                 0.85  (inH2Osat.withCO2)  (Johnson  — Ch.  News,  54,  75,  *86.) 


SILVER    CHLORATE   AgClO3. 

loo  grams  cold  water  dissolve  10  grams    AgClO3  (Vauquelin) ;  20 
gms.  AgClO3  (Wachter). 


283  SILVER    CHLORIDE 

SILVER    CHLORIDE  AgCl. 

SOLUBILITY  IN  WATER. 

(A  large  number  of  determinations  are  quoted  by  Abegg  and  Cox  —  Z.  physik.  Ch.  46,  u,  '03;  see  also 
Kohlrausch  —  Ibid.  50,  356,   04- '05;  Bottger —  Ibid.  46,  602,  '03,  56,  93,  '06.) 

t°.  I4°-  20°.  25°.  42°.  100°. 

Cms.  AgCl  per  liter      0.0014    0.0016    0.0020    0.0040    0.0218 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF: 

Ammonia  at  o°.  Mono  Methyl  Amine  at  11.5.° 

(Jarry  —  Ann.  chim.  phys.  [7]  17,  342,  '99.)  (Jarry.) 

Grams  per  100  Grams  Solution.  Gms.  per  100  Gms.  Solution. 


NH3  Gas. 

AgCl. 

NH3  Gas. 

AgCl. 

NH2CH3. 

AgCl. 

i-45 

0-49 

28.16 

6-59 

I.78 

0.16 

1.94 

I.36 

29.80 

7.09 

4-44 

0.62 

5.60 

3-44 

30.19 

7-25 

5-51 

0.83 

6.24 

4.00 

32-43 

5-87 

7.66 

1.32 

11.77 

4.68 

34  -56 

4-77 

13.70 

3-29 

16.36 

5.18 

37-48 

3-90 

18.69 

5-43 

36.69 

9-93 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 

AMMONIA. 

(Longi  —  Gazz,  chim.  ital.  13.  87,  '83;  at  25°,  Valenta  —  Monatsh.  Ch:  15,  250,  '94;  at  80°,  Pohl  — 
Sitzber.  Akad.  Wiss,  Wien,  41,  627,  '60.) 


Gms.  AgCl  per 


100 


vent. 


o  ,  *  o  Gms.  AgCl 

Solvent-  *   '  Gms.  Sol 

Aq.  Ammonia  of    o .  998  Sp.  Gr.  =  5  %  12  o .  233 

0.96    Sp.  Gr,  =  10%  18  7.84 

"                 o-986Sp.  Gr.  80  1.49 

"                                         =  3%  25  1.40 

=  15%  25  7.58 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
AMMONIUM  CHLORIDE. 

(Schierholz  —  Sitzber.  K.  Akad.  Wiss.  (Vienna)  101,  2b,  8,  '90;   see  also  Vogel  — N.  Rep.  Pharm.  23, 
335,  '74.     Hahn  —  Wyandotte  Silver  Smelting  Wks.,  1877.) 

Solubility  at  1 5°.  Solubility  at  Different  Temperatures. 

Grams  per  100  Gms.  Solution.  t  0>  Gms.  per  100  Gms.  Solution. 


NflUCl. 

AgCl. 

NH4C1.                    AgCl. 

10.00 

O.005O 

15 

26.31                 0-276 

14.29 

0-0143 

40 

0.329 

17.70 

0-0354 

60 

0-421 

19.23 

0-0577 

80 

0-592 

21.98 

o.no 

90 

0.7II 

25-31 

0.228 

IOO 

0.856 

28.45 

0-340  (24-5) 

no 

1-053 

Sat.  at  ord.  temp. 

0.157 

Sp.  Gr.  of 

26.31  %  NH4C1  solution  at 

iS°  =  i.o8. 

SILVER    CHLORIDE  284 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP 
ALUMINUM  AND  AMMONIUM  SALTS. 

(Valenta;  see  also  Cohn  —  Z.  physik.  Ch.  18,  61,  '95.) 

Cms.  AgCl  per  100  Cms.  Solvent  of  Concentration: 

Aq.  Salt  Solution.  t°.      ,  -  *  -  s 

i  :  100.  5  :  100.         10  :  100. 

Aluminum  Sutphocyanide             25  ...  ...  2.02 

Ammonium  Carbonate                  25  ...  ...  0-05 

Sulphocyanide           20  ...  0.08  0.54 

"           Thio  Sulphate            20  0.57  1.32  3.92 

"     Cak.  by  Cohn*  0.64  3.07  5.86 


*  See  Note,  p.  281. 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  HYDROCHLORIC 
ACID  SOLUTIONS  AT  ORDINARY  TEMPERATURE. 

(Pierre  —  J.  pharm.  chim.  [3]  12,  237,  '47;  Vogel.) 


Cone.  HC1  +  Aq.  5.0  100  vol.  sat.  HC1  -f  10  vol.  H2O  0.56 

i  vol.  Cone.  HC1+  i  vol.  H2O  1.6  "  +  ?o      "     "  0.18 

Sat.HCl.  Sp.  Gr.i.i6s  2.98  "  +30     "     "  0.09 

"     (atb.pt.)  5.60  "  +50     "     "  0.035 


SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Vogel;  Hahn;  Valenta ) 

Salt  Solution.  Cone,  of  Salt.  t  °.  fooGmfsofudon. 

Barium  Chloride  27.32%  24.5  0.057  (H.) 

Barium  Chloride  saturated  ord.  temp.  0.014  (Vg.) 

Barium  Sulphocyanide  10  : 100  25  0.20  (VI.) 

Calcium  Sulphocyanide  10:100  25  0.15  (VI.) 

Calcium  Chloride  41.26%  24.5  0.571  (H.) 

Calcium  Chloride  saturated  ord.  temp.  0.093  (Vg.) 

Copper  Chloride                         "  24.5  0.053  (H.) 

Ferrous  Chloride                        "  "  0.169  (H.) 

Ferric  Chloride                           "  "  0.006  (H.) 

Manganese  Chloride  0.013  (H.) 

Magnesium  Chloride  50:100  25  0.50  (VI.) 

Magnesium  Chloride  36.35%  24.5  0-531  (H.) 

Magnesium  Chloride  saturated  ord.  temp.  0.171  (Vg.) 

Strontium  Chloride  "  0.088  (Vg.) 

Zinc  Chloride  24.5  0.0134  (H.) 

Potassium  Chloride                    "  ord.  temp.  0.0475  (Vg.) 

Potassium  Chloride  24.95%  I9-^  0-0776  (H.) 

Potassium  Cyanide  5:100  25  2.75  (VI.) 

Potassium  Cyanide  5;ioo  25  5-24  (Cohn*) 

Potassium  Sulphocyanide  10: 100  25  o.n  (VI.) 

Sodium  Chloride  saturated  ord,  temp.  0-095  (Vg.) 

Sodium  Chloride  25.95%  19-6  0105  (H.) 

*  See  Note,  page  281. 


285  SILVER    CHLORIDE 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
POTASSIUM  CHLORIDE  AT  15°. 

(Schierholz  —  Sitzber.  K.  Akad.  Wiss.  (Vienna)  101,  ab,  8,  '90-) 

Grams  per  ioo  Grams  Grams  per  ioo  Grams 

Solution.  Solution. 


KC1  AgCl.  KC1.  A^CL 

lo.o  o-ooo  22.47  0-045 

14.29  O.004  24.0  O.072 

16.66  0.008  25.0  0.084 

20.00  0.020        Sp.  Gr.  of  25%  KC1  sol.,=  1.179 

MIXTURES  OF  SILVER  CHLORIDE    AND   SILVER  HYDROXIDE    IN    EQUI- 
LIBRIUM WITH  AQ.  POTASSIUM  HYDROXIDE  SOLUTIONS  AT  25°. 

(Noyes  and  Kohr  —  J.  Am,  Ch.  Soc.  24,  1144,  '02  ) 

Normality  Millimols  per  Liter  Grams  per  Liter. 

of  KOH.  KC1.  KOH.  KcT~  KOH.  ~~AgCl. 

0-333         3-4I4        347-8  0.255         10.05        0.4896 

0-065      0.598       65.0        0.0446      2-00     0-0828 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQ.  SOL.  OF  SODIUM  CHLORIDE. 

(Schierholz;  Vogel;  Hahn.) 

Solubility  Solubility  at  Different 

at  15°.  Temperatures. 

Gms.  per  ioo  Gms,  .0  Gms.  AgCl  per  ioo  Gms. 

Solution.  Solution  in: 

NaCl.  AgCl.  14%  NaCl  26.3%  NaCl. 

lo.o     0.0025        15     0.007       0.128 

14.29       0.0071  30        0-OIT  O.I32 

18.18  0-0182  40  0.014  0.158 

21.98  0-0439  50  0-023  0.184 

23.53  0.0706  70  0.042  0.263 

25.64  0.103  80  0.054  0.315 

26.31  0.127  90  0.069  0.368 

ioo  0-090  0.460 

Sp.Gr.  of  26. 31%  NaCl  sol.  =  1.207.  109  0.107(104°)     0.571 

SOLUBILITY  AT  20°,  50°,  AND  90°  (CALC.  FROM  ORIGINAL). 

(Barlow  —  J.  Am.  Chem.  Soc  28,  1446,  '06  ) 

Gms.  NaCl       Gms.  AgCl  dissolved  per  too  cc.           Gms   NaCl        Gms.  AgCl  dissolved  per  ioo  cc. 
per  ioo  cc.        Solution  at: per  ioo  cc,         Solution  at: 


Solution.         '2o°.  50°.  90°.  Solution.  2o".  50".  90", 

3.43  0.00018  0.0016  0-0067    11.5  0-0031  0.0124  0.0436 
4.60  0-00025  0.0025  o.oioo    15.3  0-0090  0.0191  0.0732 

5-75   0.00047   0.0034   0.0135      23.0   0-0313   0.0889   0.1706 
7.67   0.00125   0-0058   0-0236 

Results  are  also  given  for  the  solubility  of  silver  chloride  in  aqueous 
sodium  chloride  solutions  containing  hydrochloric  acid. 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQ.  SODIUM  NITRATE  SOLUTIONS. 

j.  o  Gms.  per  ioo  Gms.  H2O.  *  o  Gms.  per  TOO  Gms.  H2O. 

NaN03.  AgCl.    '  NaN03-  AgCl.  ' 

5     0.787   0.00086      15-20   0.393   0.00096 
18      0.787   0.00146  o  787   0.00133 

30     0.787   0.00233  2.787   0.00253 

45-55  0-787  0-00399  (Mulder ) 


SILVER    CHLORIDE  286 

SOLUBILITY  OF  SILVER  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP 
SODIUM  THIO  SULPHATE,  ETC. 

(Valenta  ;  Cohn;  Richards  and  Faber  —  Am.  Ch.  J.  21,  168,  '99.) 

Gms.  AgCl  per  100  Gms.  Aq.  Solutions  of  Concentration: 

Salt  Solution.  t°.        , ^ 

i  .  100.       5  ;  loo.       10  :  100.     15  :  100,        20  :  100. 

Sodium  Sulphite  25  ...         ...        0.44        ...  0.95 

Sodium  Thio  Sulphate  20  0.40       2.00      4.10       5 .50  6.10 

"  Calc.  by  Cohn*  0.38       1.83       3.50       5.02  6.41 

Sodium  Thio  Sulphate  35  9 .08  t 

Thio  Carbamide  25  0.83 

Thio  Cyanime  25  0.40       1.90      3-90 

*  See  Note,  page  281.  t  Gms.  per  100  cc.  solution  (R.  and  F.). 

SILVER    CHROMATE    Ag2CrO4. 

One  liter  of  water   dissolves   0.026   grn.  Ag2CrO4  at  18°,  and  0.020 

gm.    at    25°.       (Abegg  and  Cox  — Z.physik.iCh.  46,11,  '03,  Kohlrausch  —  y^^  sos  356,  '04-^5) 

SOLUBILITY  OF  SILVER  CHROMATE  IN  AQUEOUS  SOLUTIONS  OF 
NITRATES  AT  100°. 

(Carpenter  — J.  Soc.  Chem.  Ind.  5,  286,  '86.) 

o_lwr  Gms.  Salt  Gms.  Ap2CrO4 

per  100  cc.  H2O .    per  100  cc  Solution. 

Water  o  o .  064 

Sodium  Nitrate  50  0.064 

Potassium  Nitrate  50  0.192 

Ammonium  Nitrate  50  0.320 

Magnesium  Nitrate  50  0.256 

SILVER    (Di)    CHROMATE   Ag2Cr2O7. 

One  liter  of  aqueous  solution  contains  0.00019  gram  mols.  or  0.083 

gram  Ag2Cr2O7  at  15°.  (Mayer  — Ber.  36,  1741,  '03  ) 

SILVER    CITRATE    C6H5O7Ag3. 

100   gms.  H2O   dissolve  0.0277  gm.  C6H6O7Ag3  at  18°,  and  0.0284 

grn.  at  25°.  (Partheil  and  Htibner  —  Archiv.  Pharm.  241,  413,  ;o3.) 

SILVER    CYANIDE    AgCN. 

One  liter  of  aqueous  solution  contains  0.000043  grn.  AgCN  at  17.5° 
and  0.00022  gm.  at  20°  (by  Conductivity  Method). 

(Abegg  and  Cox  —  Bottger  —  Z.  physik.  Ch.  46,  602,  '03.) 

SOLUBILITY  OF  SILVER  CYANIDE  IN  AQUEOUS  AMMONIA  SOLUTIONS. 

(Longi  —  Gazz.  chem.  ital.  I3S  87,  '83.) 

ioo  gms.  aq.  ammonia  of  0.998  Sp.  Gr_  =  5%  dissolve  0.232  gm. 
AgCN  at  12°. 

ioo  gms.  aq.  ammonia  of  0.96  Sp.  Gr.  =  10%  dissolve  0.542  gm. 
AgCN  at  1 8°. 

SILVER    SODIUM    CYANIDE   AgCN.NaCN. 

ioo  gms.  H2O  dissolve  20  gms.  at  20°,  and  more  at  a  higher  tem- 
perature, ioo  gms.  85%  alcohol  dissolve  4.1  gms.  at  20°. 

(Baup  —  Ann.  chim.  phys»  [3]  53>  468,  '58.) 

SILVER    THALLOUS    CYANIDE   AgCN.TlCN. 

ioo  gms.  H2O  dissolve  4.7  gms.  at  o°,  and  7.4  gms.  at  16°. 

(Fronmiller  —  Ber    i  j,  92,  '78.) 


287  SILVER    FLUORIDE 

SILVER    FLUORIDE   AgF. 

100  gms.  H2O  dissolve  181.8  gms.  at  15.8°.     Sp.  Gr.  of  sol.  =  2.61. 

(Gore  —  Proc.  Roy.  Soc.  18,  158,  '70.) 

SILVER    FULMINATE    CAg2(NO2)CN. 

One  liter  of  aqueous  solution  contains  0.075  gm-  C2Ag2N2O2  a^  T3°» 

and  O.lSo  gm.  at  30°.  (Holleman  —  Rec.  trav.  chim.  15,  159,  '96.) 

SILVER    HEPTOATE    (Onanthylate)  AgC7H13O2. 
SOLUBILITY  IN  WATER. 

(Laudau  —  Monatsh.  Ch.  14,  709,  '93;  Altschul  —  Ibid.  17,  568,  '96.) 
f0  Gms.  AgC7Hl3O2  per  too  Gms.  H2O.          ^o  Gms.  AgC7H13O2  per  ioo  Gms.  HzO. 


O         0-0635  (Landau)  0.0436  (Altschul)      50  O  .  1652  (Landau)  o  .0858  (Altschul) 

10  0.0817  0-0494  60  0.1906  0.1036 

20  0.1007  °-°555  7°  0.2185  0.1351 

30  o.i  206  .   0.0617  80  0.2495  0.1688 

40  0.1420  0.0714 

SILVER    IODATE  AgIO3. 

One  liter  of  aqueous  solution  contains  0.04  gram  or  0.00014  g° 
mols.  at  i8°-2o°,  and  0.05334  gm.  or  0.000189  g.  rnols.  at  25°. 

(Longi;  Bottger;  Kohlrausch;  Noyes  and  Kohr  —  J.    Am.  Ch.  Soc.  24,  1141,  '02.) 

SOLUBILITY  OF  SILVER  IODATE  IN  AQUEOUS  SOLUTIONS  OF 
AMMONIA  AND  OF  NITRIC  ACID  AT  25°. 

(Longi  —  Gazz.  chim.  ital.  13,  87,  '83.) 

ioo  gms.  aq.  ammonia  of  0.998  Sp.  Gr.  =  5%  dissolve  2.36  gms.  AgIO3. 

100  gms.  aq.  ammonia  of  0.96  Sp.  Gr.  =  10%  dissolve  45.41  gms. 
AgI03. 

ioo  gms.  aq.  nitric  acid  of  1.21  Sp.  Gr.  =  35%  dissolve  0.096  gm. 
AgI03. 

SILVER    IODIDE  Agl. 

One  liter  of  aqueous  solution  contains  0.0000028  gm.  Agl  at  2o°-25°. 

(Average  of  several  determinations  by  Kohlrausch,  Abcgg  and  Cox,  etc.  Holleman  gives  higher  figures.) 

i   liter  of  aq.  ammonia  of  0.96  Sp.  Gr.  =  10%  dissolve  0.035  Srn- 

Agl  at   12°.  (Longi.) 

SOLUBILITY  OF  SILVER  IODIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Valenta  —  Monatsh.  Chem.  15,  250,  '94;  Cohn  —  Z.  physik.  Ch.  18,  61,  '95.) 

Gms.  Agl  per  ioo  Gms.  Aq.  Solution  of  Concentration: 

Aq.  Salt  Solution.  t°.     ,  --  —  ^ 

i  :  ioo.       5  :  ioo.       10  :  ioo.      15  :  ioo.        20  :  ioo. 

Sodium  Thio  Sulphate             20  0.03       0.15  0.30      0.40        0.60 

"  Calc.  by  Cohn*  0.623     2.996  5.726     8.218     10.493 

Potassium  Cyanide                   25  ...       8.28         ...... 

11  Calc.  by  Cohn*  ...       8.568       ... 

Sodium  Sulphite                       25  ...  o.oi                      0.02 

Ammonium  Sulphocyanide      20  ...       0-02  0.08       0.13 

Calcium                                     25  ...  0.03 

Barium                   "                  25  ...  0.02 

Aluminum                                  25  ...  0-02 

Thio  Carbamide                        25  ...  0.79 

Thio  Cyan  ime                          25  0.008    0.05  0.09 

*  See  Note,  page  281. 


SILVER    IODIDE  288 

SOLUBILITY  OF  SILVER   IODIDE  IN  AQUEOUS   SOLUTIONS   OF  SODIUM 
CHLORIDE,  POTASSIUM  BROMIDE  AND  OF  POTASSIUM  IODIDE  AT  15°. 

(Schierholz  —  Sitzb.  K.  Akad.  Wiss.  (Vienna)  101,  20,  10,  '90.) 

In  Sodium  Chloride.  In  Potassium  Iodide. 

Gms.  per  100  Gms.  Solution.  Gms.  per  100  Gms.  Solution. 

NaCl.  AgL KI.  Agl. 

26.31   0.0244  59 .16     53.13 

25.00   0.00072  57 .15     40.0 

50.0  25.0 

40.0  13.0 

In  Potassium  Bromide.  ^3 ' £  \'^ 

Gms.  per  100  Gms.  Solution.  25  >o  2'75 

KBr  Agl  21-74  1.576 

30.77          0.132  20. o  0.80 

TOO  gms.  sat.  silver  nitrate  solution  dissolve  2.3  gms.  Agl  at  11°, 
and  12.3  gms.  at  b.  pt. 

100  gms.  pyridine  dissolve  o.io  gm.  Agl  at  10°,  and  8.60   gms.  at 

121    .  (von  Laszcynski  —  Ber.  27,  2285,  '94.) 

SILVER    MALATE   C4H4O5Ag2. 

100  gms.  H2O  dissolve  0.0119  gm.  at  18°,  and  0.1216  gm.  at  25°. 

(Partheil    and  Hiibner  —  Archiv.  Pharm.  241,  413,  '03.) 

SILVER    NITRATE   AgNO3. 

SOLUBILITY  IN  WATER. 


(Etard  —  Ann.  chim.  phys.  [7]  2,  526,  '94;  Kramers 
Phil.  Trans 

—  Pogg.  Ann.  92,  497,  '54;  Tilden  and  Shenstone  — 
•  23,  '84.) 

to 

Grams  AgNOg  per 

100  Gms. 

to 

Grams  AgNOg  per 

100  Gms. 

. 

Solution. 

Water". 

* 

Solution. 

Water. 

-5 

48  (Etard)   .  . 

50 

79   (Etard)  82 

455 

0 

53                  55 

122 

60 

81.5            84 

525 

10 

62                  63 

170 

80 

85-5            87 

669 

20 

68            69 

222 

100 

88.5         9oi 

952 

25 

70.5        72 

257 

120 

9i            95 

1900 

30 

72-5        75 

300 

I4O 

Q3  .  "\ 

Vo    0 

AO 

76.  S            7O 

176 

1  60 

<K 

TOO  gms.  2HNO3.3H2O  dissolve  3.33  gms.  AgNO3  at  20°,  and  16.6 
gms.  at  100°. 

100  gms.  cone.  HNO3  dissolve  0.2  gm.  AgNO3. 

(Schultz  — Zeit.  Chem.  [2]  5,  531,  '69.) 

MUTUAL  SOLUBILITY  OF  SILVER  NITRATE  AND  SODIUM  NITRATE  IN 
AQ.  ETHYL  ALCOHOL. 

(Hissnik  —  Z.  physik.  Ch.  32,  5^7,  'oo.) 

Results  at  25°.  Results  at  50°. 

(In  Aq.  Alcohol  of  djo  0.945  =  37  wt.  %.)  (In  Aq.  Alcohol  of  di7  0.859  =  75  wt.  %.) 


Gms.  per  100 
Gms.  Sol. 

Wt.  per  cent  in 
Mix  Crystals. 

Gms.  per  100 
Gms.  Sol. 

Wt.  per  cent  in 
Mix  Crystals. 

AgN03. 

NaNO3. 

"AgNOs. 

NaN03. 

AgNOg. 

NaNO3. 

AgN03. 

NaNOs* 

47-32 

O-O 

100 

0.0 

29.78 

o.o 

100 

o.o 

44-01 

8.78 

99.1 

0-9 

27.9 

2-5 

99-5 

o-5 

36.78 

20.42 

42.9 

57-i 

26.4 

4-2 

99-3 

0.7 

29.97 

23.2 

33-6 

66.4 

23.0 

6-3 

42.9 

57-i 

24.56 

24.82 

27  .6 

72-4 

18-3 

7-i 

31.0 

69.0 

8.02 

26.41 

9.9 

90.1 

9-5 

8-3 

17-5 

82.5 

o-o 

26.77 

o.o 

IOO.O 

o.o 

8-54 

o.o 

100-0 

289  SILVER    NITRATE 

SOLUBILITY  OF  SILVER  NITRATE  IN  ALCOHOLS. 

(de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '92.) 

TOO  gms.  abs.  methyl  alcohol  dissolve  3.72  gms.  AgNO3  at  19°. 
100  gms.  abs.  ethyl  alcohol  dissolve  3.10  gms.  AgNO3  at  19°. 

SOLUBILITY  OF  SILVER  NITRATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Eder  — J.  pr.  Ch.  [2]  17,  45,  '78.) 

Sp.  Gr.of  Aq.        Volume  Gms.  AgNOs  per  too  Gms.  Aq.  Alcohol  at: 

Alcoholic  per  cent  t * N 

Mixture-  Alcohol.  15°.  50°.  75°. 

0-815     95       3-8      7-3      18.3 
0-863     80      10.3  42.0 

0.889        70         22.1 

0.912        60         30.5        58.1         89.0 

o-933  5o  35-8 

0.951  40  56.4     98.3     160.0 

0.964  30  73.7 

0.975  2O  107.0    214.0     340-0 

0.986  10  158-0 

100  gms.  of  a  mixture  of  i  vol.  (95%)  alcohol  +  i  vol.  ether  dis- 
solve 1.6  gms.  AgNO3  at  15°. 

100  gms.  of  a  mixture  of  2  vols.  (95%)  alcohol  +  i  vol.  ether  dis- 
solve 2.3  gms.  AgNO3  at  15°. 

100  gms.  H2O  sat.  with  ether  dissolve  88.4  gms.  AgNO3  at  15°. 

(Eder.) 

zoo  gms.  acetone   dissolve  0.35  gm.  AgNO3  at   14°,  and  0.44  gm. 

&*   J8   .  (von  Lasczynski  —  Ber.  27,  2285,  '94;  Naumann  —  Ber.  37,  4332,  '04.) 

SILVER    NITRITE    AgNO2. 
SOLUBILITY  IN  AQUEOUS  SOLUTIONS  OF  SILVER  NITRATE  AT  18°. 

(Naumann  and  Rucker  —  Ber.  38t  2293,  '05.) 
Mols.  per  Liter  Grams  per  Liter.  Mols.  per  Liter  Grams  per  Liter. 


AgNO3.           AgNO2.  AgNO3  AgNO2.  AgNO3.  AgNO2.  AgNO3.  AgNO2. 

O-OOOO  0-02067  O-OOO  3-184  0.02067  O.OI435  3-5I2  2.2OI 

0.00258  0.01975  0.439  3-°42  0.04134  o. 01168  7.024  1.799 

0.00517  0.01900  0.878  2.926  0.08268  0-00961  14.048  1.480 

0.01033  0.01689  1-756  2.601 


One  liter  of  H2O  dissolves  0.035  Sm-  at  I8°,  and  0.0365  gm.  at  20°. 

(Bottger;  Kohlrausch.) 


SILVER    OXALATE    C2O4Ag2. 
One  liter  of  H2O  dissol 

SILVER    OXIDE    Ag2O. 

One  liter  of  H2O  dissolves  0.021  gm.  at  20°,  and  0.025  gm.  at  25°. 

(Noyes  and  Kohr;  Bottger;  Abegg  and  Cox.) 

SILVER    PERMANGANATE   AgMnO4. 

100  gms.  cold  water  dissolve  0.92  gm.,  hot  water  dissolves  more. 

(Mitscherlich  —  Pogg.  Ann.  25,  301,  '39) 

SILVER    PHOSPHATE    Ag3PO4. 

One  liter  ot  water  dissolves  0.00644  grn.  at  20°. 

(Bottger  — Z.  physik.  Ch  46,  602,  '03-) 


SILVER    PROPIONATE  290 

SILVER    PROPIONATE    C2H6COOAg. 

SOLUBILITY  IN  WATERO 

(Raupenstrauch  —  Monatsh.  Ch.  6,  587,  '85;  Arrhenius  —  Z.  physik.  Ch.  11,396,  '"93;  Goldschmidt  — 

Ibid.  25,  93,  '98.) 


.  o          Gms.  C3H5O2Ag                 to 
per  Liter. 

Gms.  CsHsO^g 
per  Liter. 

to      Gms.  C3H6O; 
per  Liter. 

0 

5 

.12 

20 

8 

•36 

(8 

.48) 

50 

J3-35 

10 

6 

,78 

25 

9 

.06 

7° 

17.64 

18.2 

8 

•36 

(A.) 

30 

9 

•93 

(9 

-7o) 

80 

20.30 

SOLUBILITY  OF  SILVER  PROPIONATE  IN  AQUEOUS  SOLUTIONS  OF: 

(Arrhenius.) 

Silver  Nitrate  at  19.7°.  Sodium  Propionate  at  18.2°. 

Mols.  per  Liter.  Grams  per  Liter.  Mols.  per  Liter.  Grams  per  Liter. 


AgNOg. 

Cs^sOaAg.        AgNO3. 

C3H;02Ag. 

C3H5O2Na.    CaH5O2Ag. 

C3H6O2Na.  C3H5O2A{ 

O   0 

0 

.0471 

O 

.0 

8.519 

O 

.0 

0.0462 

O 

•  O 

8.362 

0-0133 

0 

.0415 

2 

.289 

7.511 

O 

.0167 

0-0393 

I 

.607 

7.114 

0-0267 

0 

•0379 

4 

•577 

6.86 

O 

•0333 

0.0345 

3 

•215 

6.244 

0-0533 

0 

•0307 

9 

•059 

5  -556 

O 

.0667 

0.0258 

6 

.429 

4.670 

o.ioo 

0 

.O222 

16 

•997 

4.019 

o 

•1333 

0.0191 

12 

•859 

3  .456 

o 

.2667 

0.0131 

25 

.718 

2.371 

o 

.5000 

O.OIOI 

48 

•77 

1.828 

SILVER    SALICYLATE  C6H4.OH.COOAg  1,2. 

One  liter  of  aqueous  solution  contains  0.95  gm.  at  23°. 

(Holleman  —  Z.  physik.  Ch.  12,  129,  '93.) 

SILVER    SUCCINATE    C4H4O4Ag2. 

100  gms.  H2O  dissolve  0.0176  gm.  at  18°,  and  0.0199  gm.  at  25°, 

(Partheil  and  Hiibner  —  Archiv.  Pharm.  2419  413,  '03  ) 

SILVER    SULPHATE  Ag2SO4. 

SOLUBILITY  IN  WATER. 

(Euler  —  Z.  physik  Ch.  49,  314,  '04;  Wright  and  Thomson  —  Phil.  Mag.  [5]  I7»  288,  '84;  Wentzel  — 
Dammer's  "  Handbuch  "  II,  2,  858;  Drucker  —  Z.  anorg.  Ch.  28,  362,  "oi.) 

t  °.        Gms.  Ag2SO4  per  Liter,     Gm.  Mols.  Ag2SO4  per  Liter. 

17  7.70  0.0247  (Euler.) 

18  7.28  0.0233  (W.  andT.) 

25       8.01        0.0257       (D.) 
100       14.60          ...        (W.) 

One  liter  of  aqueous  solution  in  contact  with  a  mixture  of  silver 
sulphate  and  silver  acetate  contains  3.95  gms.  Ag2SO4  +8.30  gms. 
CH3COOAg  at  17°.  Sp.  Gr.  of  solution  =  1.0094.  (Euler.) 

SOLUBILITY  OF  SILVER  SULPHATE  AT  25°  IN  AQUEOUS  SOLUTIONS  OF: 

(Drucker.) 

Sulphuric  Acid.  Potassium  Sulphate. 

Mols.  per  Liter.  Grams  per  Liter.  Mols.  per  Liter.  Grams  per  Liter. 

'Ag2SO4.        H2SO4.'  Ag7sO4.     H2SO4'.  '  Ag2SO4.       K2SO4."  Ag2SO4.     K2SO4. 

O.026o      O-O2  8. II       0.98  O.O246       O-O2  7-67          1-74 

0.0264  0-04  8.23  1.96  0.0236  0.04  7-36  3-49 
0.0271  o.io  8.45  4.90  0.0231  o.io  7.20  8.72 
0-0275  0.20  8.58  9.81  0-0232  0.20  7-24  17-44 


29I 


SILVER    SULPHATE 


SOLUBILITY  OF  SILVER  SULPHATE  AT  18°  IN  AQUEOUS     SOLU- 
TIONS OF: 

(Eder  — J.  pr.  Ch.  [2]  17,  44.  '78.) 

Ammonium  Sulphate.     Potassium  Sulphate.     Sodium  Sulphate. 


Gms.  per  100  Gms. 
Solution. 

Gms.  per  100  Gms. 
Solution. 

Gms.  per  too  Gms 
Solution. 

(NH4)aS04. 
5 
15 

Ag2S04. 

0.66 

0.85 

K2S04. 

6 
18 

Ag2S04. 
O.6o 
0.76 

Na2SO4. 
12 
32 

0.65 
0.8o 

SILVER    SULPHOCYANIDE     AgSCN. 

One  liter   of  aqueous   solution    contains  0.0002   gm.   at    25°,   and 
0.0064  gm.  at  100°. 

(Abegg  and  Cox  —  Z.  physik.  Ch.  46,  n,  '03;  Bottger  —  Ibid.  46,  60,  '05;  56,  93,  '06.) 

SOLUBILITY  OF  MIXTURES  OF  SILVER  THIOCYANATE  AND  POTAS- 
SIUM THIOCYANATE  IN  WATER  AT  25°. 

(Foote  —  Am.  Ch.  J.  30,  332,  '03.) 


Gms.  per  100  Gms.  Solution. 


Mols.  per  loo^Mols. 


KSCN. 

AgSCN. 

KSCN. 

AgSCN. 

70-53 

44-36 

66-55 

9-32 

5*  ^3 

4.19 

64.47 

10.62 

47-98 

4.6o] 

61  .25 

11.76 

42.07 

4.72  ! 

58-34 

*3-55 

38.47 

5-23T 

53-21 

17-53 

33-7i 

6.5oj 

50.68 

20.43 

32-52 

7.67 

49-43 

20.32 

30.29 

7-28] 

32-51 

18.34 

12  .26 

4-05  > 

24.68 

16.41 

7-77 

3  -02 

23.86 

16.07 

7-36 

2.90 

Solid 
Phase. 

KSCN 
KSCN  +  2KSCN.AgSCN 


Double  Salt. 

aKSCN.AgSCN  = 

53- 92%  KSCN 

2KSCN.AgSCN+ 

KSCN-AgSCN 

Double  Salt. 
KSCN.AgSCN  = 

36.9%  KSCN 

KSCN.AgSCN+ AgSCN 


SILVER    TARTRATE     C4H4O6Ag2. 

100  gms.   H2O  dissolve  0.2012  gm.   C4H4O6Ag2  at   18°,  and  0.2031 


gm.  at  25°. 


SILVER  VALERATES 


(Partheil  and  Hiibner  —  Archiv.  Pharm.  241,   413,  '03.) 


AgC5H902. 

SOLUBILITY  IN  WATER. 

Normal   Valerate  I  so  Valerate 

CH3(CH2)3.COOAg. 

(Furth  —  Monatsh.  Ch.  9,    311, 
Gms.  per  100  Gms.  HaO. 


CH3.CH(CH3)2CH2COOAg. 

Sedlitzky  —  Ibid.  8,  563,  '87.) 

Gms.  per  100  Gms.  H2O. 


*  • 

Normal  V. 

Iso  V. 

o 

0.229 

0.177 

10 

0.259 

0-2II 

20 

0-300 

0-246 

30 

0-349 

0.283 

40 

0.408 

0.321 

t    . 

Normal  V. 

Iso  V. 

50 

0-474 

0.360 

60 

o-552 

0.4OI 

70 

0.636 

0-443 

80 

0.486 

100  gms.  H2O  dissolve  0.73  gm.  silver  valerate  at  20°. 

(Markwald  —  Her.  32,  1089,  '99-) 


SILVER    VALERATE  292 

SOLUBILITY  OF  SILVER  VALERATE  IN  AQUEOUS  SOLUTIONS  OP 
SILVER  ACETATE,  SILVER  NITRATE  AND  OF  SODIUM 
VALERATE. 

(Arrhenius  —  Z.  physik.  Ch.  n   396,  '93.) 

In  Silver  Acetate  at  17.8°.  In  Silver  Nitrate  at.  16.5°. 

Mols.  per  Liter.  Gms.  per  Liter.  Mols.  per  Liter.  Gms.  per  Liter. 


C2HsO2Ag. 

C5H9O2Ag.         C2H3O2Ag.  CgHgO^ 

.g.        AgNO3.       C6HyO2Ag.          AgNO3.  ( 

o.o 

o  .  0094          o.o         i  .  96 

o.o          0.0094          o.o 

i  .96 

0.0067 

0.0070               I.I3          1.46 

0-0067       0.0068               I.I4 

1.42 

o  -0135 

0.0057               2.27          1.19 

0.0133       0.0051               2.29 

1.07 

0.0270 

0.0037               4.54         0-77 

0-0267       O.003I               4-58 

0.65 

0.0505 

0-00265            8.48         O-55 

O-IOOO      O-OOI2             17.00 

0,25 

In  Sodium 

Valerate  at  18.6°. 

Mols.  per  Liter. 

Grams,  per  Liter. 

'CjjHsOjjNa.            CsH902Ag: 

C2H302Na.       CsH902Ag. 

o.o                  0-0095 

o.o              1.986 

O.OI75                  O-OO47 

2.17                 0-982 

0-0349                  0.0030 

4.32                 0.627 

0-0698                  O-OOlS 

8.65                 0.376 

O.I395                  O.OOI5 

I7-31            0.313 

SILVER    VANADATE  Ag6V4O13. 

One  liter  of  aqueous  solution  contains  0.047  gram  at  14°,  and  0.073 

gm.  at  100°.  (Carnelly  —  Liebig's  Ann.  166,  155,  '73.) 

SODIUM    ACETATE    CH3COONa.3H2O. 

SOLUBILITY  IN  WATER. 
Interpolated  from  original. 

(Schiavor  —  Gazz.  chim.  ital.  32,  II,  532,  '02.) 
Gms.  CH3COONa  Gms.  CH3COONa 

A  o  per  TOO  Gms.  +  o  per  ioo  Gms. 

Water.    Solution.  Water.    Solution. 

o        34        25.4  25        53        34-7 

10        41        29.1  30        57        36.3 

20        49        32.9  40        65        39.4 

ioo  gms.  H2O  dissolve  46.9  gms.  CH3COONa  at  31.5°. 

(Kohler  — Z.  Ver.  Zuckerind.  47,  447,  '97.) 

ioo  cc.  aqueous  solution  contain  41.11  gms.  CH3COONa  at  10°. 

(Enklaar.) 

SOLUBILITY  OF  SODIUM  ACETATE  IN  AQUEOUS  SOLUTIONS  OF 
ACETIC  ACID. 

(Enklaar  —  Rec.  trav.  chim.  20,  183,  }oi.) 
Gram  Mols.  per  Liter.  Grams  per  Liter. 

CH3COOH."  CHgCOON'a.  CH3COOH.  CHgCOONa. 

o  5.0  o.o  411.1 

0-085  5.0  5-1  410.3 

0.12  5.0  7.2  410.4 

SOLUBILITY  OF  SODIUM  ACETATE  IN  ABSOLUTE  ALCOHOL  AT 
ROOM  TEMPERATURE. 

(Bodtker  —  Z.  physik.  Ch.  22,  510,  '97.) 

ioo  gms.  alcohol  dissolve  1.81  gms.  CH3COONa  or  7.49  gms.  CH3 
COONa.3H2O. 


293 


SODIUM    ACETATE 


SOLUBILITY  OF  SODIUM  ACETATE  IN  AQUEOUS  ALCOHOL: 
At  1 8°, 

(Gerardin — Ann.  chim.  phys.  [4]  5,  158,  '65.) 

Wt.      Gms.CHgCOONa 
per  100  Gms. 


Alcohol. 

Aq.  Alcohol. 

S-2 

38.0 

9.8 

35-9 

23.0 

29.8 

29.0 
38.0 

27-5 
23-5 

45  -° 
59-o 
86.0 

20.4 
14.6 
39 

91  .0 

2  -I 

At  Different  Temperatures. 

(Schiavor.) 

Degree           Gms.  per  100  Gms.  Alcohol. 

of                                          A 

Alcohol. 

CH3COONa. 

CH3COONa.3H20. 

8 

98.4 

2.08 

3-45 

12 

98.4 

2  .12 

3-51 

19 

98.4 

2-33 

3.86 

II 

90 

2.07 

3-42 

13 

90 

2.13 

3-52 

15 

63 

13.46 

22.32 

18 

63 

13.88 

23-03 

21 

63 

14.65 

24.30 

23 

40 

28.50 

47.27 

ioo  gms.  H2O  dissolve  237.6  gms.  sugar  +57.3  grams  CH3COONa, 
or  ioo  gms.  of  the  saturated  solution  contain  58.93  gms.  sugar  + 
14.44  gms.  CH3COONa  at  31 .  25°.  (Kohier.) 

SODIUM    ARSENATE    Na3AsO4.i2H2O. 

ioo  grams  aqueous  solution  contain  21.1  grams  Na3AsO4.i2H2O. 
(=10.4  gms.  Na3AsO4)  at  17°.  Sp.  Gr.  of  solution  =  1.1186. 

(Schiff  —  Liebig's  Ann.  113,  350,  '60.) 

ioo  grams  glycerine  dissolve  50  gms.  sodium  arsenate  at  15.5°. 

(Pharm.  Centralh.  No.  30,  '81.) 

SODIUM    HYDROGEN    ARSENATE    Na2HAsO4.i2H2O. 

ioo  gms.  H2O  dissolve  17.2  gms.  Na2HAsO4.i2H2O  (=  7.3  gms. 
anhydrous)  at  o°.  56.0  gms.  (=  19.89  gms.  anhydrous)  at  14°.  Sp.  Gr. 
1.1722,  37.0  gms.  anhydrous  at  21°,  and  140.7  gms.  hydrated  at  30°. 

(Schiff  —  Liebig's  Ann.  113,  350,  '60;  Tilden  —  J.  Ch.  Soc.  45,  409,  '84.) 

SODIUM    BENZOATE    C6H5.COONa. 

ioo  gms.  H2O  dissolve  62  gms.  at  25°,  and  77  gms.  at  b.  pt. 
ioo  gms.  alcohol  dissolve  2.3  gms.  at  25°,  and  8.3  gms.  at  b.  pt. 

(U.  s.  P.) 

SODIUM    (Tetra)    BORATE  Na2B4O7.ioH2O  (Borax). 
SOLUBILITY  IN  WATER. 

(Horn  and  Van  Wagener  —  Am.  Ch.  J.  30,  347,  '03.) 


Gms.  Na2B4O7 

Gms.  Na2B4O7 

t°. 

per  ioo  Gms. 

t  °. 

per  ioo  Gms. 

t°. 

HO. 

H20. 

5 

i-3 

5o 

10-5 

60 

10 

1.6 

54 

13-3 

62 

21.5 

2.8 

55 

14.2 

65 

30 

3-9 

56 

15.0 

70 

37-5 

5-6 

57 

16.0 

80 

45 

8.1 

90 

IOO 

Gms. 
per  ioo  Gms. 
H20. 

2O 


Transition 
imately  62°. 


19.4 

22. 0  2O-7 

22. 0  21-9 

24.4 

31-5 

41  .o 

52-5 

temperature    Na2B4O7.ioH2O  — >  Na2B4O7.5H2O   approx- 
Sp.  Gr.  of  saturated  solution  at  15°  =  1.032.        (Geriach.) 


SODIUM    BORATES  294 

SOLUBILITY  OF  SODIUM  BORATES  IN  WATER  AT  30°. 

(Dukelski  —  Z.  anorg.  Ch.  50,  42,  '06,  complete  references  given.) 


Gms.  per  ioo  Gms.  Solution. 

Gms.  per  100^ 

Gms.  Residu< 

;-             Solid 
Phase. 

K20. 

B203. 

K2O. 

B203. 

42.O 

NaOH.H2O 

41-37 

5.10 

43-54 

4.19 

" 

38-85 

5-55 

37-20 

ii.  18 

Na2O.B2O3.4H2O 

34-44 

3-73 

33-52 

10.80 

" 

29-39 

2.51 

29.63 

10.  II 

" 

26.13 

2-75 

27-85 

15.21 

" 

23.00 

3.82 

24.91 

ii  .60 

" 

16.61 

13.69 

21  .29 

20.64 

" 

21.58 

4-63 

24.52 

19.04 

Na2O.B203.4H2O  +!Na2O.B2O3.8H2O 

20.58 

4.69 

21.  6l 

16.59 

Na2O.B2O3.8H2O 

I5-32 

6.21 

19.70 

17.84 

" 

12-39 

9.12 

18.05 

18.17 

" 

8.85 

10.49 

II  .72 

20.62 

Na2O.2B2O3.ioH2O 

5.81 

6.94 

10.82 

21.31 

» 

1.88 

2.41 

7-31 

I5-50 

» 

1-38 

5  .16 

7.l6 

17.44 

«« 

2.  02 

7-79 

6.24 

16.38 

« 

4.08 

17.20 

8.96 

29.20 

Na2O.2B2O3.ioH2O  +  Na2O.5B2O3.io! 

3-79 

15.84 

5.68 

28.19 

Na2O.sB2O3.ioH2O 

2.26 

12.14 

5-21 

29.19 

H 

1.99 

11.84 

5-74 

39.66 

Na2O.2B2O3.IOH2O  +  B(OH)3 

1.86 

11.18 

i.  06 

28.78 

B(OH)3 

0.64 

6.  ii 

0.31 

3I-I9 

" 

3-54 

« 

ioo  gms.  alcohol  of  0.941  Sp.  Gr.  dissolve  2.48  gms.  sodium  borate 
at  15.5°. 

ioo  gms.  glycerine  dissolve  60.3  gms.  at  i5.5°>  and  ioo  gms.  at  80°. 

(U.S.P.) 

Gaudolphe —  J.  pharm.  chim.  [4]  22,  366,  '75  —  says  that  glycerine 
dissolves  its  weight  of  sodium  borate  at  ordinary  temperatures. 


SODIUM    BROMATE  NaBrO3. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg.  Ann.  94,  271,    55;  97,  5,  '56.) 

t°.         o°   20°    40°    60°    80°    100° 
Gms.  NaBrO3  per  ioo 

Gms.  H2O        27.5  34.5   50.2   62.5    75.7    90.9 

Sp.  Gr.  of  saturated  solution  at  19.5°=  1.231.  (Geriach.) 


295 


SODIUM    BROMIDE 


SODIUM    BROMIDE    NaBr.2H2O. 

SOLUBILITY   IN  WATER. 

(Etard  —  Compt.  rend.  98,  1432,  '84;  de  Coppet  —  Ann.  chim.  phys.  [5]  30,  411,  '83.) 


L.O                   Grams  NaBr  per  100 
Gms.  H2O. 

20 

57-5* 

7i  -4t 

O 

66 

79-5 

IO 

72 

84-5 

20 

77 

90-3 

30 

82.5 

97-3 

40 

88.0 

105.8 

t  o.        Grams  NaBr  per  100 
Gms.  H2O. 

5° 

95-112* 

n6f 

60 

112 

117 

80 

113 

119 

IOO 

114 

121 

120 

116 

124 

140 

118 

.  .  . 

*  Etard. 


t  de  Coppet. 


Transition  temperature  for  NaBr.2H2O  — »  NaBr  is  approximately 
50°.  Kremers  —  Pogg.  Ann.  97,  14,  '56  —  gives  results  which  fall  near 
those  of  de  Coppet  for  the  NaBr.2H2O,  and  near  those  of  Etard  for 
the  NaBr  section  of  the  curve. 


SOLUBILITY  OF  SODIUM  BROMIDE  IN  AQUEOUS  SOLUTIONS  OP 
SODIUM  HYDROXIDE  AT  17°. 

(Ditte  —  Compt.  rend.  124,  30,  '97.) 
Gms.  per  100  Gms.  H2O.  Gms.  per  100  Gms.  H2O.  Gms.  per  100  Gms.  H->O. 


NaOH. 

NaBr. 

NaOH. 

NaBr. 

NaOH. 

NaBr. 

0-0 

91  .38 

17.17 

63.06 

28.43 

48.00 

3.26 

79.86 

19.12 

62  .51 

36.61 

38.41 

9.24 

68.85 

22-35 

59.60 

46.96 

29-37 

13-43 

64.90 

24.74 

55-03 

54-52 

24.76 

SOLUBILITY  OF  SODIUM  BROMIDE  IN  ALCOHOLIC  SOLUTIONS. 

(Rohland  —  Z.  anorg.   Ch.  18   327,  '98;  Z.  anal.  Ch.  44,  252,  '05;  de  Bruyn  —  Z.  physik.  Ch.   10,  783 
'92;  Eder  —  Dingl.  polyt.  221,  89,  '75.) 


Alcohol. 

Methyl  Alcohol 

Ethyl 

Propyl 

Ethyl 

Methyl 

Ethyl 

Ethyl  Ether 


Concentration  «.  0 

of  Aq.  Alcohol. 

^15 ~°- 799      room  temp. 


90%  by  vol. 
Absolute 


J5 


Gms.  NaBr 

per  100  Gms. 

Alcohol. 


(R.) 


21.7 
7.14 

2  .OI 

4  .  o    (hydrated  NaBr) 
17.35         (de  Bruyn.) 
6.3    (NaBr2H20)  (Eder.) 
0.08 


SODIUM    CARBONATE 


296 


SODIUM    CARBONATE  Na2CO3.ioH2O. 

SOLUBILITY  IN  WATER. 


(Mulder;  Lowel  —  Ann.  chim.  phys.  [3]  33,  382,  '51;  at  15°,  Reich  —  Monatsh.  Ch.  12,  464,  '91;  at 
32-34.5°  Na2COa.7H2O  b,  Ketner  —  Z.  physik.  Ch.  39,  646,  'oi-'o2.) 

Solid  Phase: 
Na2CO3.ioH2O.                    Na2CO3.7H2O  (6).  Na2CO3.7H2O  (a), 

Gms.  Na2COs                                          Gms.  Na2CO3                        Gms.  Na2COa 
AO                         per  100  Gms.                                             per  100  Gms.                          per  100  Gms. 

Water. 

Solution. 

Water. 

Solution. 

Water. 

Solution. 

O 

7 

.0 

6 

•5 

20-4 

16 

•9 

32.0 

24.2 

5 

9 

•5 

6 

•9 

23-2 

18 

.8 

35-o 

25-9 

10 

12 

•5 

ii 

.1 

26.2 

20 

.8 

37-8 

27-4 

15 

16 

•4 

14 

.1 

29-5 

22 

.8 

41.2 

29.2 

20 

21 

•5 

17 

•7 

33-5 

25 

.1 

45-5 

31  -3 

25 

28 

.2  (29 

.8*) 

22  .O 

38.0 

27 

•5 

30 

37 

.8(40 

•9*) 

27 

•4 

43-5 

30 

•3 

32-5 

46 

.2 

31 

.6       (32.1 

°)46.6 

31 

.8 

35 
40 

46 
46 

.2 
.1   (49 

•7*) 

31 

.6 

(33-3 
(34-5 

°)  48.6 

32 

33 

•7 
•9 

60 

46 

.0  (46 

.4*) 

31 

.5 

Solid 

Phase  Na2CO3.H2O 

80 

45 

•8(45 

.2*) 

31 

•4 

IOO 

45 

•5 

31 

.3 

105 

45 

.2 

31 

.1 

*  Epple  —  Dissertation,  Heidelberg,  p.  26,  1899. 

Sp.  Gr.  of  solution  saturated  at  17.5°,  1.165  (Hager) ;  at  18°,  1.172 
(Kohlrausch) ;  at  23°,  1.222  (Schiff) ;  at  30°,  1.342  (Lunge).  See  also 
Wegschroeder  and  Waller  —  Monatsh.  Chem.  26,  685,  '05,  for  Sp.  Gr. 
determinations  at  other  temperatures. 


SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS 
OF  SODIUM  CHLORIDE  AT  15°. 

(Reich.) 


Gms.  per  too 
Gms.  H2O. 

Gms.  NaCl 
per  loo 

Gms.  Na2CO3 
per  loo  Gms. 

Gms.  per  loo        Gms.  NaCl  Gms.  Na2CO3 
Gms.  H2O.                   per  IOO  per  IOO  Qms. 

NaCl. 

Na2CO, 
,ioH20 

Gms. 
Solution. 

NaCl 
Solution. 

NaCl. 

Na2C03 
.ioH2O. 

Gms. 
Solution. 

NaCl 
Solution  . 

o.o 

61.42 

O 

.0 

16 

.42 

23.70 

39 

.06 

15 

.96 

9-76 

4-03 

53-86 

2 

.92 

14 

•47 

27-93 

39 

•73 

18 

.26 

9.62 

8.02 

48.00 

5 

.80 

12 

.87 

3I-65 

41 

•44 

20 

.06 

9-73 

12  .02 

43-78 

8 

.61 

II 

.62 

35-46 

43 

•77 

21 

•75 

7-95 

l6.05 

40.96 

ii 

•3i 

IO 

.70 

37-23 

45 

.27* 

22 

.46 

10.13 

19.82 

39-46 

13 

•7i 

10 

.11 

*  Both  salts  in  solid  phase. 

SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS 
OF  ETHYL  AND  OF  PROPYL  ALCOHOL  AT  20°. 

(Linebarger  —  Am.  Ch.  J.  14,  380,  '92.) 


Gms.  Na2CO3 

Gms.  Na2CO3 

Wt.  per  cent 
Alcohol. 

per  loo  Gms.  Sol. 

Wt.  per  cent 
Alcohol. 

per  loo  Gms.  Sol. 

In  Ethyl.       In  Propyi'. 

In  EthyL        In  Propyi. 

28 

4.4 

48 

0.9                    1.3 

38 

2.7 

50 

0  •  84                  1.2 

44 

1.7                    1-7 

54 

O-8o                  O-9 

46 

62 

0-4 

C2H5OH. 

Na2C03. 

H20. 

C2H5OH. 

Na2CO3. 

H2O. 

35 

62.9 

o-3 

36.8 

I  .0 

32-4 

66.6 

40 

61  .0 

0-4 

38.6 

I  .2 

31-9 

66.9 

49 

61  .0 

0-4 

38.6 

I  .2 

31-5 

67-3 

68 

55-8 

0-9 

43-3 

2-3 

28.8 

68.9 

31-2 

52-4 

0.8 

46.8 

29-3 

3r-9 

54-8 

o-7 

44-5 

i-7 

29.8 

68.5 

32-3 

56.1 

0.6 

43-3 

i-5 

30.2 

68.3 

33-2 

58.1. 

o-5 

42.4 

1.4 

31.0 

67.6 

297  SODIUM    CARBONATE 

SOLUBILITY  OF  SODIUM  CARBONATE  IN  AQUEOUS  SOLUTIONS  OF 
ETHYL  ALCOHOL. 

(Ketner  — Z.  physik.  Ch.  39,  646,  'oi-'o2.) 

NOTE.  —  The  mixtures  were  so  made  that  an  alcoholic  and  an 
aqueous  layer  were  formed,  and  these  were  brought  into  equilibrium 
with  the  solid  phase. 

Cms.  per  100  Cms.  Alcoholic  Layer.       Cms.  per  100  Cms.  Aq.  Layer. 

> * »      . * 

Phase. 

Na2C03.H20 


Na2C03.7H2O  (b) 


27.7  Crit.sol.±i4%  C2H5OH±i3%  Na2CO3±73%  H2O 

28.2         23.5         7.3         69.2  7.9         18.6         73.5        Na2C03.ioH20 

29.0        32.7         3.8         63.5  4.3         22.7         73.0 

29.7       40-0       2.1       57.9  2.9       25.5       71.6 

30.6         47.8         1.2         51.0  2.3         27.8         69.9 

SOLUBILITY  OF  Na2CO3.ioH2O  IN  DILUTE  ALCOHOL  AT  21°. 

(Ketner.) 

Grams  per  loo^Grams  Solution.  Grams  per  100  Grams  Solution. 

Na2CO3. C2H6OH.         HbO.  Na2CO3.       C2H5OH. H^O. 

18.5  o.o  81.5  1.2  39-2  59-6 

12.7  6.2  81.1  0.2  58.2  41.6 

6-9  J5-3  77-8  o.i  67.1  32.8 

3.2  26.1  70.7  0.06  73.3  26.64 

100  gms.  saturated  solution  in  glycol  contain  3.28-3.4  gms.   sodium 

Carbonate.  (de  Coninck  —  Bull.  acad.  roy.  Belgique,  359,  '05.) 

ioo    gms.  H2O  dissolve  229.2    gms.    sugar  +  24.4  gms.  Na2CO3,  or 
100  gms.  sat.  aq.  solution  contain  64.73  gms-  sugar  +  6.89  gms.  Na2CO3. 

(Kohler— Z.  Ver.  Zuckerind.  47,  447,  '97.) 

SODIUM  (Bi)  CARBONATE  NaHCO3. 

SOLUBILITY  IN  WATER. 

(Dibbits  — J.  pr.  Ch.  [2]  10,  439,  '74.) 
Gms.  NaHCO3  per  ioo  Gms  Gms.  NaHCO   per  ioo  Gms. 


i      • 

Water. 

Solution. 

Water. 

Solution 

o 

6.9 

6-5 

30 

II  .1 

IO.O 

10 

8.15 

7-5 

40 

12-7 

"•3 

20 

9.6 

8.8 

5° 

14-45 

12.6 

25 

9-4 

60 

l6-4 

13-8 

Sp.  Gr.  of  sat.  solution  at  16°  =  1.069.  (Stoiba.) 

ioo  gms.  alcohol  of  0.941  Sp.  Gr.  dissolve  1.2  gms.  NaHCO3  at  15.5°. 
ioo  gms.  glycerine  dissolve  8  gms.  NaHCO3  at  15.5°. 


SODIUM  (Bi)   CARBONATE       298 

SOLUBILITY  OF  SODIUM  BICARBONATE  IN  AQUEOUS  AMMONIUM 
BICARBONATE  SOLUTIONS  SATURATED  WITH  CO2. 

(Fedotieff  —  Z.  physik.  Ch.  49,  169,  '04.) 
«         Wt.  of  i  cc.     Mols.per  lopo  Gms.H2O.      Grams  per  1000  Gms.  H2O. 


alution. 

'  NHiHCOs. 

NaHCO3. 

NH,HC03. 

NaHC03. 

1.072 

i-39 

0.58 

109.4 

48.2 

o.o 

0.82 

o.o 

69.0 

•056 

o.o 

1.05 

o.o 

88.0 

•  O6l 

0.29 

o-95 

23.0 

80.0 

.065 

0.56 

0.89 

44-o 

74-6 

•073 

1.  08 

0.79 

85-7 

66.7 

•  090 

2.16 

0.71 

170.6 

59-2 

o.o 

1.65 

o.o 

138.6 

2.91 

0.83 

23.0 

70.0 

30 


SOLUBILITY  OF  SODIUM  BICARBONATE  IN  AQUEOUS  SOLUTIONS 
OF  SODIUM  CHLORIDE  SATURATED  WITH  CO2. 

(Fedotieff;  see  also  Reich  —  Monatsh.  Ch.  12,  464,  '91.) 


fto             Wt.  Of  I  CC. 

Mols.per  io< 

x)  Gms.HaO.       Grams  per  1000  Gms.  H2 

Solution. 

NaCl. 

NaHCO3. 

NaCl. 

NaHC03.  ' 

o 

o.o 

0.82 

o.o 

69.0 

.208 

6.0 

O.O9 

350  -1 

7-7 

15 

.056 

o.o 

1.05 

o.o 

88.0 

.063 

0.52 

0.82 

30.2 

68.6 

•073 

1.03 

0.64 

60.  1 

53-6 

tt 

.096 

2  .11 

0.41 

123.1 

34-8 

ii 

.127 

3-20 

0.28 

187.2 

23.0 

tt 

.158 

4-39 

0.19 

256-9 

16.1 

11 

.203 

6.06 

O-I2 

354-6 

10.0 

30 

.066 

o.o 

I  .31 

o.o 

IIO.  2 

.079 

I  .02 

0.87 

59-9 

72.8 

u 

.100 

2.08 

0.56 

121  .9 

47-3 

u 

.127 

3.l8 

0.38 

186.3 

32.0 

" 

.156 

0.27 

256.0 

22.3 

tt 

.199 

6.12 

0.17 

358.1 

13-9 

45 

.077 

o.o 

1.65 

o.o 

138.6 

n 

.086 

1.04 

I  .12 

60.7 

94-o 

11 

.115 

2  -65 

0.62 

155-2 

52-0 

(i 

.127 

3-24 

0.52 

189.4 

43-4 

" 

•155 

4.38 

o-37 

256.1 

30-7 

« 

.198 

6.18 

0.23 

361-5 

19.5 

loo   grams  alcohol  of  0.941    Sp.   Gr.   dissolve   5.55   grams  sodium 
sulpho  carbonate  at  15.5°. 

SODIUM    CHLORATE   NaClO3. 

SOLUBILITY  IN  WATER. 

(Kremers  —  Pogg.  Ann.  97,  4,  '56.) 

A  o  Grams  per  100  Grams  .  0  Grams  per  100  Grams 

Water.  Solution.  Water.  Solution. 

o          81.9  45 .o  60  147 .1  59.5 

12  89.3  47-2  80  175.6  63.7 

20  99-0  49-7  IOO  232.6  69.9 

40         123.5  55.3  120  333.3  76.9 


299  SODIUM    CHLORATE 

SOLUBILITY  OF  SODIUM  CHLORATE  IN  AQUEOUS  SODIUM  CHLORIDE 
SOLUTIONS  AT  20°. 

(Winteler  — Z.  Electrochem.  7,  360,  'oo.) 

Volume  Wt.  Grams  per  Liter.  Volume  Wt.  Grams  per  Liter. 

of  Solutions.  NaCL          NaClOa.  of  Solutions.  NjJcT  NaClOa- 

1.426  5  668  1.365  175  393 

1.419  25  638  1.345  200  338 

1.412  50  599  1.319  225  271 

1.405  75  559  1.289  250  197 

1.398  loo  522  1.256  275  120 

1.389  125  484  1.235  290  78 

1.379  150  442  1.217  300  55 

loo  gms.  H2O  dissolve  24.4  gms.  NaCl  +  50.75  gms.  NaClO,  at  12°. 

loo  gms.  H2O  dissolve  11.5  gms.  NaClH-  249.6  gms.  NaClO3  at  122°. 

(Schlosing  — Compt.  rend.  73»  1273.  *7i-) 

loo  gms.  alcohol  of  77  Wt.  per  cent  dissolve  2.9  gms.  NaClO3  at  16°. 

(Wittstein.) 

loo  gms.  alcohol  dissolve  i  gm.  NaClO3  at  25°,  and  2.5  gms.  at  b.  pt. 
loo  gms.  glycerine  dissolve  20  gms.  NaClO8  at  15.5°. 

SODIUM    CHLORIDE    NaCl. 

SOLUBILITY  IN  WATER. 

(Mulder  ;  de  Coppet  —  Ann.  chim.  phys.  [5]  30,  411,  '83;  Andrae  —  J.  pr.  Ch.  [2]  29,  456,  '84;  above 
100°,  Tilden  and  Shenstone  —  Phil.  Trans.  23,  '84;  Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203  A,  206, 
'04;  Etard  —  Ann.  chim.  phys.  [7]  2,  527,  '94,  gives  irregular  results.) 

to         Gms.  NaCl  per  Gms^NaCl  Gms.  NaCl  per  Gms-Naa 

iooGms,H20.  joo^Sol  IPO  Gms.  H2O.  ^^ 

o  35-7*  35-63t  26.28!  70  37-3*  37-51!  27^ 

10  35 -8  35-69  26.29  80  38.4   38.00  27.54 

20  36.0  35.82  26.37  90  39.0   38.52^  27.80 

25  36-12  35.92  26.43  zoo  39.8   39-12!  28.12 

30  36.3  36.03  26.49  II8       39-8  28.46 

40  36.6  36.32  26.65  I4°       42.1  29.63 

50  37-o  36-67  26.83  160       43-6  30.37 

60  37-3  37-o6  27.04  180       44.9  30-98 

*  M.;  de  C.  t  A.  t  B. 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP 
AMMONIUM  CHLORIDE. 

(Fedotieff  —  Z.  physik.  Ch.  49,  170,  '04.) 

o          Wt.  of  i  cc.  Mols.  per  1000  Gms.  H2O.  Grams  per  1000  Gms.  H2O. 

Solution.  '  NH4C1.  NaCl!  NH4C1. NaCl'. 

o  ...  o.o  6.09  o.o  356.3 

"  1-185  2-73  4.89  I46.I  286.4 

15    1.200       o.o      6.12        o.o     357-6 
1.191       1.07     5.58       57.3     326.4 

"  I-l83  2.22  5.13  Il8-9  3OO.O 

"  I.I76  3-48  4-64  186.4  271.6 

"  I.I75  3.72  4.55  198.8  266.8 

30           ...  o.o  6.16  o.o  360.3 

1.166  4.77  4-26  255.4  249.0 

45     ...  o.o  6.24  o.o  365-0 

"     ...  6.02  4.0  322.1  233.9 


SODIUM    CHLORIDE 


300 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROCHLORIC  ACID. 

(Engel  —  Ann.  chim.  phys.  [6]  13,  374,  '88;  Enklaar  —  Rec.  trav.  chim.  20,  183,  'or.) 

At0.  .(Engel.)                                    At  io°-io.5°.   (Enklaar.) 

Mg.  Mols.  per  10  cc.       Sp.  Gr.  of           Gms.  per  Liter.               Mols.  per  Liter.           Grams  per  Liter. 

HC1. 

NaCl. 

Solution. 

HCl. 

NaCl. 

HCl. 

NaCl.' 

HCl. 

NaCl. 

o.o 

54-7 

I 

.207 

O 

•  O 

32.0 

o.o 

6.  ii 

o 

•  O 

35-77 

I  .0 

53-5 

j 

204 

0 

•365 

31-3 

0.27 

5-77 

9 

.84 

33-76 

1.85 

52.2 

j 

•  2O2 

O 

.674 

30-5 

o-35 

5-67 

12 

>76 

33-19 

5-1 

48-5 

I 

.196 

I 

•859 

28.4 

o-43 

5-59 

15 

.68 

32.71 

9.28 

44.0 

I 

.185 

3 

•38 

25-7 

o-57 

5-43 

20 

.78 

31-77 

J5-05 

37-9 

I 

•173 

5 

•49 

22.2 

0.72 

5-28 

26 

.06 

30.89 

30-75 

23-5 

I 

.141 

ii 

.20 

13-7 

2  .60 

3-42 

94 

•77 

20.  01 

56-35 

6.1 

I 

.119 

20 

•54 

3-6 

2.8o 

3.18 

IO2 

.1 

19.04 

3-31 

2.74 

120 

.6 

16.03 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  CHLORIDE  AND  OTHER 
SALTS  IN  WATER,  ETC. 

Gms.  per  100  Gms.  Solvent.  Authority. 

(Karsten.) 


(Soch  — J.  Physic.  Ch.  2,  46,  '98.) 


(Quoted  by  Euler  — Z.  physik.  Ch. 
49,  3i5.  '04.) 

*  Sp.  Gr.  of  solution  at  17°  =  1.179. 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  CHLORIDE  AND  POTASSIUM 
SULPHATE  IN  WATER  AT  VARIOUS  TEMPERATURES. 

(Precht  and  Wittgen  — Ber.  15,  1666,  '82.) 


Solvent. 

t  °. 

Water 

17 

u 

17 

u 

p 

It 

25 

(I 

80 

Alcohol  (40%) 

25 

Water 
« 

20 

Of* 

17 

t  — 
26 

•4 

NaCl+22.iNH4Cl* 

17 

34 

•5 

u 

+   4.iBaCl2 

? 

38 

3 

Cl 

+  29.5KN03 

25 

38 

5 

(t 

+  41-14     "       . 

80 

39 

,81 

(t 

+  168.8     " 

25 

J5 

.78 

(t 

+  13-74     " 

20 

30 

54 

(I 

+  I3-95KC1  j, 

25 

28 

.90 

(I 

+  16.12     "     J 

^o          Grams  per  ipo 

Grams  H2O.          t  o 

Grams  per  100  Grams  H2O. 

'   NaCl 

K2S04 

KU 

NaCl 

K2S04 

KCt 

10 

33-4 

8 

.1 

3 

.2 

60 

36 

•4 

II 

•9 

2-7 

20 

34-o 

8 

9 

3 

.1 

70 

36 

.6 

12 

.8 

3-2 

30 

34-6 

9 

.6 

2 

•9 

80 

36 

.0 

12 

•3 

5.1 

40 

35-2 

10 

•4 

2 

.8 

9o 

35 

•9 

12 

•4 

7-o 

50 

35-8 

ii 

.1 

2 

.8 

IOO 

35 

.6 

12 

.6 

8.8 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  BICARBONATE  SATURATED  WITH  CO2. 

(Fedotieff.) 

Grams  per  10000  Gms.  H2O. 


«.o          Wt.  Of  I  CC. 

Mols.  per  1000 

Gms.  Hj 

Solution. 

NaHC03. 

NaCl. 

0 

O-O 

6.09 

<t 

.208 

0-09 

6.0 

15 

.203 

o.o 

6.12 

tt 

.203 

0.12 

6.06 

30 

.196 

o.o 

6.16 

.199 

0.17 

6.12 

45        1.189 

0-0 

6.24 

1.198 

0.23 

6.18 

NaHCO3. 

NaCl. 

O-O 

356.3 

7-7 

350-1 

o.o 

357-6 

10.  0 

354-6 

o.o 

360.3 

13  9 

358.1 

0-0 

•3  cj  6  .  o 

0.23 

361  .  i\ 

3oi  SODIUM    CHLORIDE 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SODIUM  HYDROXIDE 

SOLUTIONS. 

(Engel;  Winteler  —  Z.  Electrochem.  7,  360,  Joo.) 

At  o°  (Engel).  At  20°  (Winteler). 


Mg.Mols 

.  per  10  cc. 

Sp.  Gr.  of 

Grams  per  Liter. 

Gms.  per  Liter 

Sp.  Gr.  of 

Na2O. 

NaCl. 

Solutions. 

NaOH. 

NaCl. 

NaOH. 

NaCl. 

Solutions. 

0 

54 

.7 

I 

.207 

0 

.0 

320 

.0 

10 

308 

I  .200 

4-8 

49 

•38 

I 

.221 

38 

•4 

288 

•9 

50 

297 

1.230 

6-73 

47 

.21 

I 

•225 

53 

.8 

276 

.2 

IOO 

253 

I  .250 

10.41 

42 

-38 

I 

-236 

183 

.2 

247.9            I5° 

2I3 

I  .270 

14-78 

39 

•55 

I 

.249 

118 

.2 

231 

•4 

2OO 

139 

I-305 

30.50 

24 

•95 

I 

•295 

244 

.0 

146 

.0 

300 

112 

37-88 

19 

•30 

I 

•314 

303 

.0 

112 

9 

40O 

6l 

i-375 

53-25 

9 

.41 

I 

.362 

426 

.0 

55 

.0 

500 

30 

1.425 

640 

18 

1.490 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  NITRATE  AND  VICE  VERSA. 

(Bodlander  —  Z.  physik.  Ch.  7,  361,  '91;   Nicol  — Phil.  Mag.  [5]  3L  369,  '91;  results  at  25°  by  Soch  — 

J.  Physic.  Ch.  2,  46,  '98.) 

NaCl  in  Aqueous  NaNO3.  NaNO3  in  Aqueous  NaCl. 

Results  at  15.5°  (B.).  Results  at  15°  (B.). 


Sp.  Gr.  of 

Gms.  per 

ioo  cc.  Sat.  Solution. 

Sp.  Gr.  of 

Gms.  per 

ioo  cc.  Sat 

.  Solution. 

Solutions. 

NaN03. 

H20. 

NaCl. 

Solutions. 

NaCl. 

H2O. 

NaNOs. 

I  .2025 

O 

88-47 

31 

.78 

I 

.3720 

0 

74.82 

62.38 

I-2305 

7 

•53 

87.63 

27 

.89 

I 

•3645 

4 

.0 

75-69 

56.76 

1.2580 

13 

.24 

86.25 

26 

•31 

I 

•3585 

7 

.24 

75-71 

52.09 

I  .2810 

21 

•58 

82.66 

23 

.98 

I 

•3530 

ii 

•36 

76.86 

47-oS 

1.3090 

28 

.18 

80.42 

22 

•30 

I 

•3495 

15 

•33 

76.96 

42.66 

*-3345 

33-80 

79-25 

2O 

.40 

I 

•3485 

i7 

.81 

77-14 

39-90 

1-3465 

37 

.88* 

77-37 

19 

.40* 

I 

•3485 

18 

-97* 

77-15 

38.73* 

1-3465 

37 

,64* 

77-34 

J9 

.e?* 

I 

•3485 

19 

•34* 

77-49 

38.02* 

Results  at  20°  (N.). 

Grams  per  ioo  Grams  H2O.  Grams  per  ioo  Grams  H2O. 


o        NaNO3  35.91  NaCl  o  NaCl       87.65  NaNO3 

14.17  32.82      "  6.5  77.34 

28.33  29.78  13.0  68.50 

42.50        "  26.91  19.5  60.49 

54.63*      "  24.92* 

ioo   gms.   H2O   dissolve   43.66*  gms.    NaNO3  +  26.58*  gms.    NaCl 
at  25°. 

ioo  gms.  H2O  dissolve  121.6*  gms.  NaNO3  +  17.62*  gms.   NaCl  at 

80°. 

ioo  gms.  aq.  alcohol  of  40  wt.  per  cent  dissolve  22.78  gms.  NaNO,  -f 
10.17  gms.  NaCl  at  25°. 

*  Indicates  solutions  saturated  with  both  salts. 


SODIUM    CHLORIDE  302 

SOLUBILITY  OF  SODIUM  CHLORIDE  IN  ALCOHOLS. 

(At  18.5°,  de  Bruyn  —  Z.  physik.  Ch.  10,  782,  '92;  Rohland  —  Z.  anorg.  Ch.  i89  327,  '98.) 

Gms.  NaCl  Cms.  Nad 

t°.  Alcohol.  per  100  t°.  Alcohol  per  100 

Gms.  Alcohol.  Gms.  Alcohol. 

18.5      Abs.  Methyl      1.41         room  temp.     Methyl  d15= 0.799      1.33 
"     Ethyl        0.065  Ethyl  d15    =0.81        0.176 

"  Propyl  d15  =0.816      0.033 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  ETHYL  ALCOHOL 

SOLUTIONS. 

(Bodlander  —  Z.  physik.  Ch.  7t  317,  '91;  Taylor  —  J.  Phys.  Ch.  i,  723,  '97;  also  Bathrick  —  Ibid.  I, 

159.  '96.) 

Results  at  11.5°  (B.).  Results  at  13°  (B.). 


Sp.  Gr.  of 

Gms.  per  100  cc.  Solution. 

Sp.  Gr.  of 

Gms.  per  100  cc.  Solution. 

Solutions. 

C2H6OH. 

H2O. 

NaCl. 

Solutions. 

C2H5OH. 

H20. 

NaCl. 

1-2035 

o 

86 

.62 

31 

•73 

1.2030 

0 

88.70 

31.60 

1.1865 

2 

.86 

86 

.14 

29 

.66 

I  .  1348 

II 

.81 

78.41 

23.26 

.1710 

5 

.41 

83 

•93 

27 

•77 

I.II44 

IS 

99 

74.64 

20.  8l 

.1548 

7 

•93 

81 

•5o 

26 

•05 

I  .0970 

19 

39 

7r-45 

18.86 

•1350 

10 

.84 

78 

•78 

24 

.28 

1.0698 

24 

95 

69.80 

16.23 

.1390 

n 

.22 

78 

.62 

23 

65 

1.0295 

32 

33 

57-96 

12.66 

.1088 

16 

•85 

73 

.40 

20 

63 

0.9880 

40 

33 

49-34 

9-J3 

0-9445 

49 

28 

38-54 

5-93 

0.9075 

57 

91 

29-37 

3-47 

0.8700 

63 

86 

21  .62 

1.52 

o  .  8400 

72 

26 

II  .24 

0.50 

Results  at  30°  and  at  40°  (T.). 

Wt   per  cent        At  30°.  Gms.  NaCl  per  100  Gms.  At  40°,  Gms.  NaCl  per  ipoGms. 

Alcohol  in  Solvent.      Solution.  Water.  '     Solution.  Water. 

o  26.50  36-05  26.68  36-38 

5  24.59  34-29  24.79  34-69 

10  22.66  32-57  22.90  33 .00 

20  I9-°5  29.40  19.46  30.20 

30  15.67  26.53  16.02  27.25 

40  12.45  23-7o  12.75  24.37 

50  9.34  20.60  9.67  21.42 

60  6.36  16.96  6.65  17.82 

70  3.36  12.75  3-87  13  ^o 

80  1.56  7.95  1.69  8.68 

90  0.43  4-3°  °-5°  5-10 

100  gms.  alcohol  of  0.9282  Sp.  Gr.  =  54.0%  by  wt.  dissolve  at: 

4°       10°       13°         23°       32°       33°       44°       5i°       °o° 
10.9     ii. i     11.43     n-9     I2-3     I2-5     I3-1     T3-8     14-1  gms.  NaCl 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  146,  '56.) 

ioo  gms.  of  a  mixture  of  equal  parts  of  96%  alcohol  and  98%  ether 
dissolve  o.n  gm.  NaCl. 

(Mayer  —  Liebig's  Ann.  98,  205,  '56.) 


303 


SODIUM    CHLORIDE 


SOLUBILITY  OF  SODIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
Acetone  at  20°.  Glycerine  at  25°. 

(Herz  and  Knoch  — Z.  anorg.  Ch.  41,  318,  '04.)  (H.  and  K.  —  Ibid.  45,  267,  '05.) 


cc.  Acetone 
per  loo  cc. 

NaCl  per  100 
cc.  Solution. 

Wt.  per  cent          NaCl  per  100 
Glycerine  in              cc.  Solution 

Sp.  Gr.  of 

Solvent. 
O 

Millimols.    Grams. 

537-9    3J-47 

Solvent. 

o.o 

Millimols. 

545-6 

Grams'.    * 
31.93           .1960 

10 

464 

.6 

27 

18 

13.28 

i 

29.31 

.2048 

20 

394 

.8 

23 

10 

25.98 

448 

4 

26 

23 

•2133 

30 

330 

.1 

19 

32 

45-36 

37o 

2 

21 

66 

•2283 

32 

)  Lower  layer 

308 

•5 

18 

05 

54-23 

333 

9 

J9 

54 

•  2381 

87 

i  Upper  layer 

7 

•7 

0 

•45 

83.84 

220 

8 

12 

91     1.2666 

88 

7 

•3 

o 

43 

100.00* 

167 

.1 

9 

.78    1.2964 

90 

4 

•3 

o 

25 

*Sp.  Gr. 

of  Glycerine, 

1.2592. 

Impurities  about  1.5%. 
100  gms.  sat.  solution  in  glycol  contain  31.7  gms.  NaCl  at  14.8°. 

(de  Coninck  —  Chem.  Centralb.  76,  II,  883,  '05.) 

zoo  gms.  H2O  dissolve  236.3  gms.  sugar  +  42.3  gms.  NaCl  at  31.25°, 
or  100  gms.  sat.  aq.  solution  contain  62.17  gms.  sugar  4-  11.13  gms- 

NaCl.  (Kohler  —  Z.  Ver.  Zuckerind.  47,  447,  '97.) 


SODIUM    CHROMATES   (Mono,  Di,  etc.) 

SOLUBILITY  IN  WATER. 

(Mylius  and  Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  451,  'oo;  see  also  Salkowski  —  Ber.  34,  1948,  *oi.) 


Sodium  Mono  Chromate. 


Sodium  Di  Chromate. 


Gms.  Na2 
to           Cr04per 
100  Gms. 

Mols.  Na2 
CrO4  per         Solid 
100  Mols       Phase. 

f. 

Gms.  Na2    Mols.  Na2 
Cr2O7  per     Cr2Oy    per               Solid 
100  Gms.       loo  Mols.                Phase. 

Solution. 

H20. 

Solution.        H2O. 

O 

24.07 

3  •52Na2CrO4.ioH^ 

0     O 

61.98       1  1.  2           Na^r^r.aEbO 

IO 

33-41 

5-55 

17 

63.82       1  2.  1 

18* 

40.IO 

7-43 

i8J 

63.92     12.  16 

18.5 

41.65 

7-94 

34-5 

67.36       14.2 

19-5 

44.78 

9.01 

52 

71.76       17.4 

21 

47-40 

10-00 

72 

76.9         22.8 

25.6 

46.08 

9.52Na2CrO4.4H2C 

>  81 

79-8         27.1 

3*  -5 

47-05 

9.90 

93 

81.19      29.6                 Na2Cr2O7 

36 

47.98 

10-2 

98 

81.25       29.8 

40 

48.97 

10.6 

/• 

Sodium  Tri  Chromate. 

A£ 

so  .20 

ii  .6             " 

"J 

0 

Gms.  Na2   Mols.  Na2 

49-5 

50-93 

11.5 

to 

Cr3O,0  per  Cr3Oi0  per                Solid 

54-5 

52.28 

12.2                  " 

• 

100  Gms.     100  Mols.               Phase. 
Solution.        H2O 

59-5 

53-39 

12-7 

0 

80.03       *9   9           Na2Cr3Ol0.H2O. 

65 

55-23 

13-7          Na2Cr04 

I5t 

80  .  44     20.4 

7o 

55-J5 

I3.6 

18 

80-60      20.56 

80 

55-53 

I3.8 

55 

82.68      23.7 

100 

55-74 

I4.O 

99 

85.78      29.9 

*Sp.  Gr.  of  sat.  sol.  at  18°  =  1.432.   tSp.  Gr.  of  sat.  sol.  at  18°  =  2.059. 
jSp.  Gr.  of  sat.  solution  at  18°  =  1.745. 


SODIUM    CHROMATES                3 

Sodium  Tetra  Chromate. 

tv 

Gms. 

per  ioo  Gms. 
Solution. 

Mols. 
Na2Cr4OJ3 
per  ioo 
Mols.H20. 

Solid 
Phase. 

o 
16 

18* 

22 

72.96 
74.19 
74.60 
76.01 

10-5 
II  .2 
II  .27 
I2.3 

Na2Cr40,3.4H20 

M 

3°4 


Tetra  Sodium  Chromate. 


Gms.  Mols. 

Na4CrO5     Na4CrO6 
per  ioo  Gms.     per  ioo 


10 

i8f 

27.7 

37 


Solution. 

35-58 
37-50 
40.09 

45:i3 


Viols.  H2O. 
4-II 
4.42 
4.8l 

5-38 
6.62 


Solid 
Phase. 


*  Sp.  Gr.  of  sat.  solution  at  18°=  1.926. 


t  Sp.  Gr.  of  sat.  solution  at  18°  =  1.446. 


SOLUBILITY  OF  SODIUM  CHROMATES  IN  WATER  AT  30°. 

(Schreinemaker  —  Z.  physik.  Ch.  55,  91,  '06.) 

Composition  in  weight  per  cent : 
Of  Solution.  Of  Residue. 


%Cr03- 

%Na20. 

%Cr03. 

%Na20. 

Solid  Phase. 

O 

±42 

.  .  . 

NaOH.H2O 

2  .OO 

41.44 

5*83 

42.64 

NaOH.H2O  +  Na2CrO4 

2.04 

40-89 

.  .  . 

Na2Cr04 

4-23 

35-51 

27.52 

36.57 

" 

6.64 

32-34 

27.72 

34.60 

" 

IS  -!9 

27.06 

37-07 

32.20 

" 

IO.22 

29-39 

I5-48 

28.41 

Na2CrO4  +  Na4CrO6.i3H2O 

8-93 

28.49 

18.09 

26.89 

Na4CrO6.i3H20 

8.62 

26.91 

" 

13.12 

23.91 

18.57 

25.92 

«« 

18.44 

22.86 

.  .  . 

it 

19.26 

22.98 

21.54 

25-3I 

N^CrOs.isH-zO  +  Na2CrO4.4H2O 

17.84 

24.21 

26.24 

24-98 

Na2Cr04.4H2O 

28.82 

17.88 

31-97 

23-47 

" 

38.93 

16.30 

40.70 

20-83 

" 

48.70 

16.49 

47-49 

19-75 

Na2CrO4.4H2O  +  Na2Cr2O7.2H2O 

50.68 

15-72 

Na2Cr207.2H2O 

58.08 

13.89 

62.76 

I7-38 

" 

66.13 

13.70 

69.48 

16.06 

Na2Cr2O7.2H2O  +  Na2Cr3Oio.H2O 

65.98 

J4-I5 

69.46 

I5-I5 

Na2Cr3O10.H20 

68.46 

10.95 

73-88 

I3-38 

Na2Cr3Oio.H2O  +  Na2Cr4Ql3-4H2O 

66.88 

9-85 

71.27 

10.67 

Na2Cr3O,3.4H2O 

70.06 

11.85 

83-95 

9-57 

"  (?) 

69.04 

ii  .04 

81.80 

6-43 

CrOa 

67.84 

9.81 

82.85 

5-42 

« 

64.48 

4-5i 

79-49 

2.71 

«« 

62.28 

o.o 

100.00 

" 

ioo  gms.  of  a  saturated  aqueous  solution  contain  at  30°: 
46.627  gms.  Na2CrO4,  or  ioo  gms.  H2O  dissolve  87.36  gms.  Na-jCrO,. 
66.4  gms.  Na2Cr2O7,  or  ioo  gms.  H2O  dissolve  197.6  gms.  Na2Cr2O7. 
ioo  gms.  absolute  methyl  alcohol  dissolve  0.345  gm.  Na2CrO4  at  25°. 

(de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '93.) 


305  SODIUM    CITRATE 

SODIUM    CITRATE    2C3H4(OH)(COONa)3.nH2O. 

100  gms.  H2O  dissolve  90.9  gms.  citrate  at  25°,  and  250  gms.  at  b.  pt. 

(U-S.P.) 

SODIUM  (Ferro)    CYANIDE   Na4Fe(CN)6. 

SOLUBILITY  IN  WATER. 

(Conroy  —  J.  Soc.  Chem.  Ind.  17,  104,  '98.) 

t°  20°.  42°.  80°.  98.5°. 

Gms.  Na4Fe(CN)6  per  ioo  gms.  H2O          17.9      30.2       59.2       63.0 
SODIUM    FORMATE   HCOONa,     SOLUBILITY  IN  WATER. 

(Groschuff  —  Ber.  36,  1788,  '03.) 

Gms.  Mols.  Gms.  Mols. 

to        HCOONa    HCOONa  Solid  to  HCOONa    HCOONa  Solid 

'   per  ioo  Gms.  per  ioo  Mols.  Phase.  periooGms   per  ioo  Mols.        Phase. 

Solution.          H2O.  Solution.          H2O. 

—  20      22.8o  7.82       HCOONa.sH2O       25.5       50.53         27.0        HCOONa.aH2O 

O      30.47         II. 6  "  l8  49.22         25    65         HCOONa 

+  15      41.88         19.1  29  50.44         26.9 

18     44.92       21.6  "  54        53.80      30.8 

l8      44-73         21-4         HCOONa.2H2O       74.5      56.82         34.8 

21     46.86       23.3  100.5     6l-54      42-35 

23     48.22       24.65  123         66.20       51-8 

Sp.  Gr.  of  the  saturated  solution  of  the  dihydrate  at  18°  =  1.317. 

SOLUBILITY  OF  SODIUM  ACID  FORMATE  (EXPRESSED  AS  NEUTRAL 
SALT)  IN  AQUEOUS  SOLUTIONS  OF  FORMIC  ACID. 

(Groschuff.) 

Gms.  Mols.  Gms.  Mols. 

to         HCOONa    HCOONa  Solid  to       HCOONa    HCOONa         Solid 

'     per  ioo  Gms.  per  ioo  Mols.  Phase.  *     per  ioo  Gms.  per  ioo  Mols.    Phase. 

Solution.          H2O.  Solution.         H2O. 

O  22.35         19.5  HCOONa-HCOOH        45.5      38.85         43.1        HCOONa 

25.5  29.62   28.45  7°    41-27   47-5 

66.5  41.08   47.1  85    43 .09   51.2 

SODIUM    FLUORIDE    NaF. 

ioo  gms.  sat.  aq.  solution  contain  4.3  gms.  NaF  at  18°.     Sp.  Gr.  of 

Solution  =    1.044.  (Mylius  and  Funk  — Ber.  30,  1718,  '97.) 

SOLUBILITY  OF  SODIUM  FLUORIDE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROFLUORIC  ACID  AT  21°. 

(Ditte  —  Compt.  rend.  123,  1282,  '96.) 
Grams  per  1000  Grams  H^.  Grams  per  1000  Grams  HgO. 

o.oHF~  41. 7  NaF  83.8  HF  22.9  NaF 

io. o    "  4i-4     "  129.7    "  23.8     " 

45.8    "  22.5     "  596.4    "  48-8     " 

56.5    "  22.7     "  777-4    "  8i-7     " 


SODIUM    FLUO    SILICATE   Na2SiF6. 

ioo  gms.  H2O  dissolve  0.65  gin.  at  17.5°,  and  2.45  gms.  at  100°. 

(Stolba  — Z.  anal.  Ch.  n,  199,  '72.) 


SODIUM    HYDROXIDE 


306 


SODIUM    HYDROXIDE    NaOH. 

SOLUBILITY  IN  WATER. 

(Pickering  —  J.  Ch.  Soc. 63,  890,  '93;  Mylius  and  Funk  (Dietz)  —  Wiss.  Abh.  p. t.  Reichamstalt  3,  450,  'oo.) 


Gms.  NaOH 
to            per  ioo  Gms. 

Solution. 

Water. 

-  7.8 

8.0 

8.7 

—  20 

16.0 

19.1 

-28 

19.0 

23-5 

—  24 

22.2 

28-5 

-17.7 

24-5 

32-5 

0 

29.6 

42  .O 

+  5 

32.2 

47-5 

10 

34-o 

51  .5 

15-5 

38-9 

63-53 

5 

45-5 

83-5 

12 

50.7 

103.0 

Solid 
Phase. 


Ice 


Ice  +  NaOH.7H2O 
NaOH.7H20  +  NaOH.SH2O 
NaOH.5H20  +  NaOH^HijO  a 
NaOH.4H20  a 

NaOH.4H20  a+  NaOH3iH2O 
NaOH.3iH2O 

f.  pt. 

NaOH.aiHjsO  +  NaOH.2H.zO 
NaOH.2H20  +  NaOH.H20 


20 

30 

40 
50 
60 


80 
no 

192 


Gms.  NaOH 
per  ioo  Gms. 

Solid 
Phase. 

NaOH.H2O 

Solution. 
52.2 

Water. 

109 

54-3 
56.3 

119 
129 

« 

59-2 
63-5 

i74 

M 

69.0 

74.2 

222.3 

288 

NaOH^H20 
+  NaOH 

75-8 
78.5 

313 
365 

NaOH  (?) 

83  -9 

521 

Sp.  Gr.  of  sat.  solution  at  18°  =  1.539. 

For  determinations  of  the  Sp.  Gr.  of  sodium  hydroxide  solution,  see 
Kohlrausch  —  Wied.  Ann.  i,  1879;  Wegschnider  and  Waller  — 
Monatsh.  Chem.  26,  685,  '05. 

SODIUM    IODATE    NaIO3. 

SOLUBILITY  IN  WATER. 

(Gay-Lussac;  Kremers  —  Pogg.  Ann.  97,  5,  '56.) 
t°.  o°.  20°.        40°.  60°  80°.        100°. 

Gms.  NaIO3  per  ioo  gms.  H2O   2.5    9    15    21    27    34 

SODIUM    IODIDE    NaI.2H2O. 

SOLUBILITY  IN  WATER. 

(de  Copper  —  Ann.  chim.  phys.  [5]  30,  411,  '83;  see  also  Etard  —  Compt.  rend.  98,  1434,  '84;  and  Kremers 

—  Pogg.  Ann.  97,  14,  '56.) 


t° 

Grams  Nal 

per  ioo  Gms.       Solid 

t° 

Grams  Na! 

[  per  ioo  Gm 

's-         Solid 

Water. 

Solution.         Phase. 

Water. 

Solution. 

Phase. 

—  20 

148.0 

59  .  7     NaI.2H2O 

60 

256.8 

72.0 

NaI.2H2O 

O 

158.7 

61.4 

65 

278.4 

73-6 

" 

10 

168.6 

62.8 

67 

293 

74.6 

Nal 

2O 

178.7 

64  .  1 

70 

294 

74.6 

" 

25 

184.2 

64.8 

80 

296 

74-7 

" 

30 

190.3 

65.6 

IOO 

302 

75  .1 

" 

40 

205.0 

67.2            <f 

120 

3IO 

75-6 

" 

50 

227.8 

69.5 

I4O 

321 

76-3 

" 

SOLUBILITY  OF  SODIUM  IODIDE  IN  SEVERAL  SOLVENTS. 

(At  22.5°,  de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '92;  at  ord.  temp.,  Rohland  —  Z.  anorg.  Ch.  18,  327,  '98; 
Walden  —  Z.  physik.  Ch.  55,  713,  718,  '06.) 

Gms.  Nal 

_  .  Gms-  Nal  .  .  per  too  Gms. 

Solvent.  t  .  per  ioo  Solvent.  Solution. 

Gms.  Solvent.  > — 

at 

Absolute  Ethyl  Alcohol 
d, 5  0.8 10  Ethyl  Alcohol 
Absolute  Methyl  Alcohol 
d15  o.  799  Methyl  Alcohol 
dls  0.816  Propyl  Alcohol 


VJIHS.  ouiveiu 
22.5                      43.1 

ord.  temp.     58.8 
22.5               77.7 
ord.  temp.     83.3 
ord.  temp.     26.3 

Acetonitril 
Propionitril 
Nitro  Methane 
Acetone 
Furfurol 

at  o°.       at  25°. 
22.09      18.43 
9.09         6.23 
0.34        0.48 

very  soluble 
25.10 

SODIUM    MOLYBDATE 


SODIUM    MOLYBDATE    Na2MoO4. 

SOLUBILITY  IN  WATER. 


4 
6 

9 

10 


Cms. 
Na2MoO4 
per  100 
Cms. 
Solution. 


35-58 
38.16 
39.28 


Mols. 
Na2MoO4 
per  100 

Mols. 

H20. 


(Funk  —  Ber.  33,  3697,  'oo.) 


Solid 
Phase. 


3.86Na2Mo04.ioH20    15.5 

4-47  18 

4-83  32 

5-39  5i-5 

5  .65  Na2MoO4.2H2O  IOO 


Cms. 
Na2Mo04 
per  loo 
Cms. 
Solution. 

Mols. 
Na2MoO4 
per  TOO 
Mols. 
H20. 

Solid 
Phase. 

39-27 

5  .65  Na2Mo04.2ll2O 

39-40 
39.82 
41.27 

5-70 
5-78 
6.14 

„ 

45-57 

7-32 

11 

zoo  gms.  H2O  dissolve  3.878  gms.  sodium  tri  molybdate  Na2Mo3O10 
at  20°,  and  13.7  gms.  at  100°. 

(Ullik  —  Liebig's  Ann.  144,  244,  '67.) 


SODIUM    NITRATE  NaNO3. 


SOLUBILITY  IN  WATER. 


(Mulder;  Berkeley  —  Trans.   Roy.  Soc.  (Lond.)  203  A,  211,  '04;  see  also  Ditte  —  Compt.  rend.  80,  1164, 
'75;  Maumee — Ibid.  58,  81,  '64;  Etard  —  Ann.  chim.  phys.  [7]  2,  527,  '94.) 

Gms.  NaNO3  per  100  Gms.     Mols.  per 


to 

Gms.  NaNO3  per  100  Gms. 

Mols.  per 

t° 

• 

Solution. 

Water. 

Liter. 

0 

42.2 

72.9-    73.0* 

6.71* 

80 

IO 

44-7 

80.8-   80.5 

7.l6 

IOO 

20 

46.7 

87.5-  88.0 

7.6o 

120 

25 

47.6 

91.0-  92.0 

7.8o 

180 

30 

48.7 

94.9-  96.2 

8.06 

220 

40 

50-5 

102.0-104.9 

8.51 

225 

50 

52.8 

112.0-114.0 

8.97 

313 

60 

54-9 

122.0—124.0 

9.42 

Solution.  Water.  Liter. 

7      148.0-148.0*   10.35* 
3       180.0-175.8     11.30 

68.6         2l8. 0-208. 8t    I2.22f 

i  356-7 
5  5o6-o 
5  1076.0 

00 


59- 
64. 


78. 
83. 


pt.  100.0 


*  Berkeley. 


t  "9° 


SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF 
NITRIC  ACID  AT  o°. 

(Engel  —  Compt.  rend.  104,  911,  '87;  see  also  Schultz  —  Zeit.  Ch.  [2]  5,  531,  '62.) 
Equivalents  per  10  cc.  Solution, 


NaN03. 

HNO3. 

66.4 

O 

63-7 

2  .65 

60.5 

5-7 

56-9 

8.8 

52-75 

12-57 

48-7 

16.9 

39-5 

27.0 

35-1 

32-25 

31-1 

37-25 

23-5 

48.0 

18.0 

57-25 

12.9 

71.0 

p.  Gr.  of 

Grams  per  i 

oo  cc.  Solution. 

olutions. 

NaNO3. 

HN03. 

I-34I 

56.5 

O-OO 

I-338 

54-2 

1.67 

51.48 

3-59 

•324 

48.42 

5-55 

.312 

44-88 

7-92 

.308 

41.44 

10.65 

.291 

33  -6l 

17.02 

.285 

29.86 

20-33 

.282 

26.46 

23-48 

I  .276 

20.  o 

30.26 

I  .276 

I5-32 

36.09 

I  .291 

10.97 

44.76 

SODIUM    NITRATE  308 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  NITRATE  AND  POTASSIUM 
NITRATE  IN  WATER  AT  20°. 

(Carnelly  and  Thomson  —  J.  Ch.  Soc.  53,  709,  '88.) 

NaNC^n  Gms'  *F  '°°  Gms'  NaNcSn  Gms"  P«  '°°  Gms' 

Mixtures  H2°- t  Mixtures  HzP- _ 

Used.  NaNO3.  KNO3.  Used.  NaNO3.  KNOa. 

ioo  86.8  o  45-7  53-3  34-7 

90  96.4  13.2  40  45-6  35-5 

80  98.0  38.5  20  20.8  33.3 

60  90.0  47.6  10  9.4  31.5 

50  66.  o  40.0         o  o.o  33-6 

ioo  gms.  H2O  dissolve  24.9  gms.  NaCl  +  53.6  gms.  NaNO3  at  20°. 

(Rxidorff  —  Ber.  6,  484,  '73;  Karsten;  Nicol  —  Phil.  Mag.  [5]  31,  386,  '91.) 

SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF 
•     SODIUM  HYDROXIDE  AT  o°. 

(Engel  —  Bull.  soc.  chim.  [3]  6,  16,  '91.) 

Milligram  Mols.  per  10  Sp.  Gr.  Grams  per  ioo  cc. 

cc.  Solution.  of  . Solution. 

Na2O. NaNOjj,"  Solutions.  NaOH. NaNO3'. 

o.o  66.4  1-341  o.o  56-50 

2.875       62.5  1.338  2.30        53.19 

6.1  57-15  1-333.  4-89  48-63 

12.75  47-5  J-327  10-21  40-42 

26.0  29.5  1.326  20.83  25.10 

39-o  17-5  •      x-332  3I-25  J4.89 

45.88  13.19  1.356  36.76  11.22 

60.88  6.05  1.401  48-75  5-15 

SOLUBILITY  OF  SODIUM  NITRATE  IN  ALCOHOLS. 

ioo  gms.  abs.  methyl  alcohol  dissolve  0.41  gm.  NaNO3  at  25°. 
ioo  gms.  abs.  ethyl  alcohol  dissolve  0.036  gm.  NaNO3  at  25°. 

(de  Bruyn  —  Z.  physik.  Ch.  10,  783,  '92.) 

SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  ETHYL  ALCOHOL 
AT  DIFFERENT  TEMPERATURES. 

(Bodlander  —  Z.  physik.  Ch.  7,  317,  '91;  Taylor — J. Physic.  Ch.  i,  723,  '97;  Bathrick — Ibid.  I,  i62,"'96,) 


Results  at  13°  (B.). 

Sn  Gr  of           Gms.  per  ioo  cc.  Solution. 

Results  at  16.5°  (B.). 

So  Gr.of       Gms.  per  ioo  cc.  Solution. 

Solutions. 

C6H6OH. 

H20. 

NaN03. 

Solutions. 

C6H5OH. 

H20. 

NaNO3. 

1.3700 

0 

.0 

75-34 

61 

.66 

I 

•3745 

o.o 

75 

•25 

62  -2O 

1-3395 

3 

.08 

73-53 

57 

•34 

I 

.3162 

6.16 

70 

.82 

54-64 

1.3120 

6 

.01 

71.81 

53 

•39 

I 

.2576 

II  .60 

68 

.10 

46.06 

1.2845 

8 

•30 

70.85 

49 

•30 

I 

.2140 

16.49 

65 

.04 

39-87 

i  .2580 

10 

.91 

69.47 

45 

.42 

I 

.1615 

22.17 

61 

.67 

32-31 

1-2325 

13 

•77 

67.12 

42 

•36 

I 

•0855 

32.22 

52 

.92 

23-4I 

i  .2010 

16 

.46 

66.16 

37 

.48 

I 

•0558 

37-23 

48 

•50 

19.85 

I 

.0050 

43-98 

42 

.78 

13-74 

O 

.9420 

52.60 

32 

•13 

9-47 

O 

.9030 

6o.OO 

25 

•65 

4-65 

0 

.8610 

63.16 

21 

•31 

1.63 

3°9 


SODIUM    NITRATE 


Results  at  30°  (T.). 


Wt.  per  cent 
Alcohol  in 

Gms.  NaNO3 
per  ioo  Gms. 

Solvent. 

Solution. 

Water- 

O 

49-10 

96-4S 

5 

46.41 

9I-I5 

10 

43-50 

85-55 

20 

37-42 

74-75 

30 

3I-3I 

65.10 

40 

25.14 

55-95 

50 

18.94 

46.75 

60 

12-97 

37-25 

70 

7.8l 

28.25 

90 

I  .21 

12  .25 

Results 

at  40°. 

(Bathrick.) 

Wt. 
•per  cent 
Alcohol. 

Cms.  NaNOa 
per  ioo  Gms. 
Aq.  Alcohol. 

O 

104-5 

8.22 

90-8 

17.4 

73-3 

26.O 

6l.6 

36.0 

48.4 

42.8 

4O.6 

55-3 

27.1 

65.1 

18.1 

77.0 

9-4 

87.2 

4.2 

SOLUBILITY  OF  SODIUM  NITRATE  IN  AQUEOUS  SOLUTIONS  OF 

ACETONE. 
Results  at  30°. 

(Taylor.) 


Results  at  40°. 

(Bathrick.) 


Wt.  per  cent 
Acetone  in 

Gms.  NaNO3 
per  ioo  Gms. 

Solvent. 

Solution. 

Water. 

0 

49-10 

96.45 

5 

46.96 

93-20 

9.09 

45  -11 

90.40 

2O 

40.10 

83.70 

30 

35-o8 

77-20 

40 

29.80 

70-75 

50 

24-34 

64.40 

60 

18.55 

59-95 

70 

13  .15 

50-50 

80 

7.10 

38-20 

90 

1.98 

20.20 

Wt. 

per  cent 
Acetone. 

O-O 
8.47 

16.8 

25.2 

34-3 
44-i 

53-9 
64.8 
76.0 
87.6 


Gms.  NaNOa 
per  ioo  Gms. 
Aq.  Acetone. 


91 

78. 


66.4 

57-9 
46.2 
32.8 
23.0 
10.8 
3-2 


SODIUM    NITRITE    NaNCX. 

ioo  gms.  H2O  dissolve  83.3  gms.  at  15°. 

(Divers  — J-  Ch.  Soc.  75,  86-  '00} 

ioo  gms.  abs.  methyl  alcohol  dissolve  4.43  gms.  NaNO2  at  19.5°. 
ioo  gms.  abs.  ethyl  alcohol  dissolve  0.31  gm.  NaNO2  at  19.5°. 

(de  Bruyn  —  Z.  physik.  Ch.  10,  783,    92.) 

SODIUM    RHODO    NITRITE    Na6Rh2(NO2)12. 

ioo  gms.  H2O  dissolve  40  gms.  at  17°,  and  ioo  gms.  at  100°. 

(Leidie  —  Compt.  rend.  HI,  107,  '90.) 


SODIUM    OXALATE    C2O4Na2. 

SOLUBILITY  IN  WATER. 

(Souchay  and  Leussen  —  Liebig's  Ann.  99,  33,  '56;  Pohl  —  J.  pr.  Ch.  56,  216,  '52.) 
t°.  15.5°.  21 3°.  100°. 

Gms.  Na2C2O4  per  ioo  gms.  H2O        3.22        3 . 74        6 .33 


SODIUM    OXALATE  310 

SOLUBILITY  OF  MIXTURES  OP  SODIUM  OXALATE  AND  OXALIC 
ACID  IN  WATER  AT  25°. 

(Foote  and  Andrew  —  Am.  Ch.  J.  34,  154.  '°S-) 

Gms.  per  100  Gms.  Mols.  per  too  Mols. 

Solution.  H2Q. 

Na2C204.      H2C204.    Na2C2O4. 


IO-2O  ...  2  .274  .  .  .  H2C2O4.2H2O 

10.50  0.83  2.370  0.130  H2C2O4.2H20+HNaC2O4.H2O 

9.15  0.71  2.032 


0.47       3.  20          0.098 

0.42  3.85  0-090          0.541  HNaC2O4.H2O  +  Na2C2O4 

3  .  60  ...  O  •  502  Na2C2O4 

SODIUM    p    NITRO    PHENOL  C6H4.ONa(i).NO2(4). 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  NORMAL  SOLUTIONS  OP 
NON  ELECTROLYTES. 

(Goldschmidt  —  Z.  physik.  Ch.  17,  154,  '95.) 

Gms.  C6H4.ONa(i).NO2(4)  per  100  Gms.  Solution  in: 


23-7 
28.6 

•70  6 

Water. 

5-597 
6.721 

7   2<?6 

Alcohol. 

5-6l5 
6.874 

Urea. 
6.244 

7.489 

Glycerine. 
6.188 
7.440 

Acetone. 
6.225 

7.498 

Propionitril. 
6.257 

7-571 

Acetonitril 
6.065 
7.328 

.   Urethane. 
6.520 
7.889 

JO.U 

33-6 

35-9 
36.1 
40.2 
45-2 
50-i 

/  "^0^ 

8.125 
8.851 

8.883 
9.881 

"•235 
12.730 

8.318 

10.147 
"-5!3 
I3-I33 

9.OOO 
9.683 

10.666 
12.068 
13-555 

9.025 

9.688 
10.777 
12.  229 
13.785 

9.025 

9.665 
10.695 

9.066 

9.911 
10.905 

8.886 

9.667 
10.667 

9-507 
10.248 

n-379 
12.869 

The  solid  phase  is  C6H4ONa.NO2.4H2O  below  36°,  and  C6H4ONa. 
NO2.2H2O  above  36°  in  each  case. 

SODIUM    PHOSPHATES,  Ortho,  Hydrogen,  and  Pyro. 
SOLUBILITY  OF  EACH  IN  WATER. 

(Mulder;  Poggiale.) 
-o  Gms.  per  100  Gms.  Water.  |.o  Gms.  per  100  Gms.  H2O. 

NasPCv Na2HP04. Na4P267.  Na3PO4.     Na2HPo7         Na^CV 

o    1.5    2.5    3.16      40    31.0    63.9    13.50 
10    4-1    3-9    3-95      50    43-o    82.5    17.45 

20     II. O      9-3     6.23         60      55-0     91.6     21.83 

25    15.5    15-4    8.14      80    81.0    96.6    30.04 
30    20. o    24.1    9-95     100    108.0    99 -o    40.26 

Solid  phases,  Na3PO4.i2H2O,  Na2HPO4.i2H2O  and  Na4P2O7.ioH2O 
respectively.  Sp.  Gr.  of  saturated  solution  of  Na2HPO4  at  15°=  1.047., 

100  gms.  alcohol  of  0.941  Sp.  Gr.  dissolve  0.33  gm.  sodium  phos- 
phate at  15.5°. 

SODIUM  (Double)   PHOSPHATE,   FLUORIDE  Na3PO4.NaF.i2H2O. 

100  gms.  water  dissolve  12  gms.  of  the  double  sodium  salt  at  25°, 

and  57.5  gms.  at  70°.     Sp.  Gr.  of  solution  at  25°=  1.0329;  at  70°= 

I.IOQI.  (Briegleb  —  Liebig's  Ann.  97-,  95.  's<5.) 


SODIUM    PHOSPHITES 


SOLUBILITY  OF 

Salt. 

Hydrogen  Phosphite 


Hypophosphate 
Hydrogen  Hypophosphate 
Tri  Hydrogen       " 
Di  Hydrogen        " 
Di  Hydrogen         " 
Hypophosphite 
Hypophosphite 


SODIUM  PHOSPHITES,  ETC.,  IN  WATER. 

Formula.  t".     per  100  Cms.  Authority. 

(NaH)HPO3.2iH20   o 

10 

42 

Na4P206.ioH20 
Na3HP206.9H20 
NaH3P2063H20 
Na2H2P206.6H20 
Na2H2P2O6.6H2O 
(NaH)HPO2.H2O 
(NaH)HPO2.H2O 


(Amat. —  Compt. 
rend.  106,  1351,  '88.) 


(Salzer  —  Liebig's 
Ann.  an,  i,  '82.) 

1  (Salzer  —  Liebig's 
\  Ann.  187,  331,  '77.) 

(U.  S.  P.) 


SODIUM    SELENATE   Na2SeO4.ioH2O.     SOLUBILITY  IN  WATER. 

(Funk  —  Ber.  33,  3697.  'oo.) 


Gms.  Mols. 

Na2SeO4  per   Na2SeO4 


I  . 

ioo  Gms. 

ioo  Mol 

Solution. 

H20. 

o 

11-74 

I  .26 

15 

25  .OI 

3  •I^ 

18 

29.00 

3-9o 

25.2 

36.91 

5-57 

27 

39.18 

6.13 

30 

44-05 

7  -5° 

Solid 
Phase. 


Na2SeO4.ioH2O 


Gms.  Mols. 

Na2Se04  per  Na2SeO4  per        Solid 
100  Gms.        100  Mols.          Phase. 


NajSeO* 


Solution. 

HzO. 

35-2 
39-5 

45-47 
45.26 

7-94 
7.87 

75 

IOO 

44-49 
42.83 
42.14 

7.14 
6-93 

Sp.  Gr.  of  saturated  solution  at  18°  =  1.315. 

SODIUM    STANNATE   Na2SnO3.3H2O. 

ioo  gms.  H2O  dissolve  67.4  gms.  at  o°,  and  61.3  gms.  at  20°.     Sp. 
Gr.  of  solution  at  o°  =  1.472;  at  20°=  i.438- 

(Ordway  —  Am.  J.  Sci.   [2]  40,  173,  '65.) 


SODIUM    SULPHATE   Na2SO4.    SOLUBILITY  IN  WATER, 

(Mulder;  Lowel  —  Ann.chim.  phys.  [3] 


35,  345.   '83;  Etard  —  Ann.  chim.  phys.  [7]  2,  527,  '94;  Funk  —  Ber.  33,  3?oi, 
Roy.  Soc.  (Lond.)  203  A,  209,  '04.) 

Gms.  Na2S04  per        Mols.                                         Gms-  N*2SO<  I*r 
t°.                 ioo  Gms.         Na2S04per        Solid             t°-           ioo  Gms.            j 

'oo;  BerJ 

Mols. 
<a?S04p 

Solution. 

Water. 

Liter  (B.)- 

Solution. 

Water.      ^»er  u 

O 

4 

.76 

5 

.0 

0.31    Na2SO4.ioH 

2°      5O 

31- 

8 

46. 

7 

2.92 

5 

6 

.0 

6 

•4 

" 

60 

31- 

2 

45 

3 

2.83 

10 

8 

•3 

9 

.0 

0.631         " 

80 

30- 

4 

43 

•7 

2.69 

15 

ii 

.8 

13 

•4 

" 

IOO 

29. 

8 

42 

•5 

2.60 

20 

16 

•3 

19 

•4 

1.32 

1  20 

29. 

5 

41 

•95 

25 

21 

•9 

28 

•  o 

.  .  . 

140 

29 

6 

42 

27-5 

25 

.6 

34 

.0 

...            " 

160 

30 

•7 

44 

•25 

30 

29 

.0 

40 

.8 

2  .  63 

230 

31 

•7 

46 

•4 

30 

.6 

44 

.0 

.  .  . 

o 

16 

•3 

19 

•5 

32 

32 

•3 

47 

.8 

...            ' 

5 

19 

4 

24 

32-75 

33-6 

50 

•65 

3  -11 

10 

23 

.1 

30 

33 

33 

.6 

50 

.6 

.  .  .    Na£O4 

15 

27 

.0 

37 

35 

33 

•4 

50 

.2 

...           " 

20 

30 

.6 

44 

40 

32 

.8 

48 

.8 

3-01 

25 

34 

.6 

53 

Na,S04 


Na2S04.7H20 


SODIUM    SULPHATE  312 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  SULPHATE  AND  MAGNESIUM 
SULPHATE  IN  WATER  (ASTRAKANITE)   Na2Mg(So4)2.4H2o. 

(Roozeboom  —  Rec.  trav.  chim.  6,  342,  '87;  Z.  physik.  Ch.  2,  518,  '88.) 

Solid 
Phase. 

Astrakanite 


Astrakanite  -f  Na 


Astrakanite  +  MgSO4 


Mols. 

per  100 

Grams  per 

100 

t°. 

Mols. 

H20. 

Grams  H2O. 

Na2SO4. 

MgSO4. 

Na2SO4. 

Mgso4: 

22 

2 

•95 

4 

.70 

23-3 

31 

•4 

24 

•5 

3 

•45 

3 

.68 

27.2 

24 

.6 

30 

3 

•59 

3 

•59 

28.4 

24 

.1 

35 

3 

•7i 

3 

•7i 

29.4 

24 

.8 

47 

3 

.6 

3 

.6 

28.4 

24 

.1 

22 

2 

•95 

4 

.70 

23-3 

31 

•4 

24 

•5 

3 

•45 

3 

.62 

27.2 

24 

.2 

30 

4 

•58 

2 

.91 

36.1 

J9 

.1 

35 

4 

•3 

2 

.76 

33-9 

18 

•44 

18 

•5 

3 

.41 

4 

.27 

43-o 

45 

•5 

22 

2 

•85 

4 

•63 

35-2 

48 

•9 

24 

•5 

2 

.68 

4 

.76 

32-5 

5o 

•3 

30 

2 

•3 

5 

•3i 

25-9 

55-o 

35 

I 

•73 

5 

.88 

23-5 

59 

•4 

SOLUBILITY  OF  MIXTURES  OF  SODIUM  SULPHATE,  POTASSIUM 
CHLORIDE,  POTASSIUM  SULPHATE,  ETC.,  IN  WATER. 

(Meyerhoffer  and  Saunders  —  Z.  physik.  Ch.  28,  469;  31,  382,  '99.) 


t< 

> 

Sp.  Gr.  of 

Mols.  per  1000  Mols.  H2O. 

. 

* 

Solutions. 

S04 

K2 

Na2 

C12 

Solid  Pha.sc. 

*4- 

4 

5- 

42 

14. 

39 

51- 

83 

60. 

8 

K3Na(S04)2+Na2SO4.ioH2O+ 
KCl-}-NaCl 

0. 

2 

3- 

35 

12. 

78 

5° 

93 

60. 

36 

Na2S04.ioH20+KCl+NaCl 

—  o. 

4 

3- 

59 

16. 

38 

40. 

75 

53-54 

Na2SO4.ioH2O+KCl+K3Na(SO4)2 

16. 

3 

4- 

72 

17- 

58 

50. 

56 

63- 

42 

K3Na(SO4)2+KCl+NaCl 

24. 

8 

I  .  2484 

4- 

37 

20. 

00 

48. 

36 

64. 

01 

K3Na(SO4)d-KCl+NaCl 

*i6. 

3 

16. 

29 

9- 

16 

61. 

06 

53- 

93 

K3Na(S04)2+NaCl+Na2SO4.ioH2O+ 

24. 

5 

1.2625 

14. 

45 

9- 

90 

58. 

46 

53- 

9i 

K3Na(S04)24-NaCl+Na2S04 

0. 

3 

2. 

75 

25- 

77 

17. 

93 

40.95 

K3Na(S04)2+KCl+K2S04 

25- 

0 

I  .  2034 

2. 

94 

36. 

20 

14. 

80 

48. 

06 

K3Na(S04)2+KCl+K2SO4 

*i7: 

9 

1.2474 

13.84 

0. 

0 

62.57 

48. 

70 

Na2S04.ioH2O+Na2SO4+NaCl 

*3o. 

i 

I  .  2890 

50- 

4i 

10. 

08 

40. 

33 

0. 

0 

K3Na(SO4)2+Na2S04.ioH2O+Na2SO4 

—  21. 

4 

. 

. 

46. 

61 

46. 

36 

NaCl  .2H2O+Na2SO4.ioH2O 

-23- 

7 

. 

10. 

51 

39- 

58 

50. 

09 

NaC1.2H2O+KCl 

—  10. 

9 

I. 

45 

30. 

68 

29. 

23 

KC1+K2SO4 

-  3 

16. 

25 

10. 

03 

6. 

21 

K3Na(SO4)2+Na2SO4.ioH2O 

-  3 

16. 

24 

IO. 

03 

6. 

21 

. 

K3Na(S04)2-r-K2S04 

-14 

i. 

39 

25- 

59 

8. 

78 

32- 

94 

K3Na(SO4)2+Na2SO4  .1  oH2O+KCl 

-14 

i. 

39 

25- 

59 

8. 

78 

32- 

94 

K3Na(SO4)2+K2SO4+KCl 

-23- 

3 

0. 

15- 

44- 

20 

58. 

97 

Na2SO4.ioH2O+KCl+NaC1.2H2O 

*  Indicates  transition  points. 


3*3 


SODIUM    SULPHATE 


SOLUBILITY  OF  SODIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OP 
SULPHURIC  ACID. 

(D'Ans,  Shepherd  and  Giinther —  Z.  anorg.  Chem.  49,  356-61,  '06.) 


Cms.  per  1000  Cms.  Solution.    Mols.  per  1000  gms.  Solution 


H,S04 

Na2S04 

H2SO4 

Na2S04 

0.0 

2IQ.O 

0.0 

I.54I 

28.1 

237-4 

0.286 

1.671 

33-2 

247-5 

0.338 

1.742 

86.7 

320.7 

0.884 

2.256 

154.6 

335-8 

1.576 

2.363 

163.5 

346.4 

1.666 

2-437 

256.3      297.4 


Solid  Phase. 


Na2SO4  •  10  H20 


Na2S04  •  10  H2O  +  Na2S04 

Na3H(S04)  -H20  +  Na2SOi 
Na3H(SO4)2+Na2S04 
2.611        2.091     Na3H(SO4)2  +  Na3H(S04)2  -  H2O 


SOLUBILITY  OF  SODIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS  OF 
SODIUM  CHLORIDE  AT  DIFFERENT  TEMPERATURES. 

(Seidell  — Am.  Ch.  J.  27,  52,  '02.) 


Results  at  10°. 


Results  at  21.5' 


Results  at  27°. 


Sp.  Gr.    Gms.  per  100  Gms. 
of                     H2O. 

Sp.  Gr.      Gms.  per  100  Gms. 
of                     H20. 

Sp.  Gr.        Gms.  per  100  Gms. 
of                        HaO- 

Solutions.    NaCl.    Na2SO4." 

Solutions.       Nad.        Na2SO4.' 

Solutions.        Nad.      NaabCv 

.080      o.o      9.14 

1.164      o.o       21.33 

1.228       o.o       31-10 

.083         4.28      6.42 

1.169      9-05     x5-48 

1.230       2.66     28.73 

.IO2         9.60      4-76 

1.199    17.48    13.73 

.230         5.29       27.17 

•150     J5-65     3-99 

1.214     20.41     13-62 

.235      7  .90    26.02 

.164     21.82     3.97 

1.243    26-01    15.05 

.259     16.13     24.83 

1.192     28.13     4-i5 

1.244    26.53    14.44 

.253     18.91     21.39 

1.207     30-11     4-34 

1.244   27.74    13.39 

.249     19.64    20.  i  i 

1.217     32.27     4.59 

1.244    3*-25     10.64 

.245     20.77     *9-29 

1.223     33.76    4.75 

1.243     31.80     10.28 

•238    32-33      9-53 

1.245    32.10     8.43 

1.219   33.69     4.73 

I.  212       34.08          2.77 

1.197     35-46      o.oo 

Results  at  30°. 

Results  at  33°. 

Results  at  35°. 

Sp.  Gr.         Gms.  per  TOO  Gms. 
of                         H2O. 

So  Gr        Gms.  per  100  Gms. 
of     '                   HzO. 

Sp.  Gr.      Gms.  per  100  Gms. 
of                       H2p- 

Solutions.      NaCl.       Na2SO4. 

Solutions.      NaCl.         Na2SO4. 

Solutions.    Nad.          Na2SO 

1.281       o.o      39-7o 

1.329      o.o      48.48 

.324      o.o      47-94 

1.282      2.45    38.25 

1.323          1.22       46.49 

.314      2.14    43.75 

1.284     5.61    36.50 

1.318      1.99    45  .16 

.256     13-57     26.26 

1.290     7.91   35.96 

1.315          2.64      44-09 

.238     18.78     19.74 

1.276     10.61     31-64 

1-309      3-47     42-6i 

.231     31.91       8.28 

1.270    12.36    29.87 

1.265     12.14    29-32 

•193     35-63       o.oo 

1.258    15.65    25.02 

1.237     21.87     l6-83 

1.249     18.44     21.30 

1.234    32.84      8.76 

1.244     20.66     19.06 

1-217     33-99      4-63 

1.236   32.43     9.06 

1.208    34.77       2.75 

SODIUM    SULPHATE 

SOLUBILITY  OF  SODIUM  SULPHATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(de  Bruyn  —  Z.  physik.  Chem.  32,  101,  *oo.) 


Content     Gms.  Na2SO4 
t°.               of          per  100  Gms. 
Alcohol.     Aq.  Alcohol. 

Gms. 

per  100  Gms.  Solution. 

Solid 
Phase. 

'H2O. 

C2H6OH.    Na2SO4. 

IS 

0.7 

12.7 

88.7 

o.o 

"•3 

Na2SO4.ioH2O 

tt 

9.2 

6.7 

85.I 

8.6 

6-3 

" 

a 

19.4 

2.6 

78.6 

18.9 

2.9 

" 

(i 

39-7 

0.5 

00.0 

39-5 

0.5 

" 

n 

58-9 

O.I 

4I.I 

58.8 

O.I 

" 

tt 

72.0 

o.o 

28.0 

72.0 

o.o 

" 

it 

o.o 

37-4 

72.8 

o.o 

27.2 

Na2S04.7H20 

tt 

II  .2 

16.3 

76.5 

9-5 

14.0 

" 

tt 

20.  6 

7.0 

74-3 

19.2 

6-5 

" 

cc 

30.2 

2  .O 

68.4 

29.6 

2  .O 

" 

25 

o.o 

28.2 

78.1 

o.o 

21-9 

Na2SO4.ioH2O 

tt 

10.6 

13-9 

78.5 

9-3 

12  .2 

" 

(t 

24.0 

4-5 

72.8 

22  .9 

4-3 

" 

(I 

54-o 

0.4 

45-6 

54-o 

0.4 

" 

36 

o.o 

49-3 

67.0 

o.o 

33-o 

Na2S04 

tt 

8.8 

29.2 

70.6 

6.8 

22.6 

tt 

12.8 

22.4 

71.2 

10.5 

I8.3 

« 

tt 

17.9 

15-4 

71.1 

13-4 

« 

ft 

18.1 

15-3 

71.0 

J5-7 

13-3 

« 

It 

28.9 

5-4 

66.5 

28.4 

5-1 

» 

tt 

48.7 

0.8 

50-9 

48.3 

0.8 

« 

45 

o.o 

47-9 

67.6 

o.o 

32-4 

» 

tt 

9.0 

27-5 

71  .3 

7-1 

21.6 

« 

tt 

14-5 

19.2 

71.8 

12.  1 

16.1 

•« 

tt 

20.  6 

12.3 

70.6 

18.4 

10-  O 

« 

tt 

31.0 

65.6 

29-5 

4-9 

* 

Between  certain  concentrations 

of  the  aqueous 

alcohol  the  liquid 

separates  into  two  layers  at 

25°,  36 

0  and  45°. 

o 

Upper  Layer. 

Lower  Layer. 

Gms.HaO. 

Gms.CuHgOH. 

Gms.Na2SO4.        Gms.H2O.    Gms,C2H5OH.  Gms.Na2SO4 

25 

66.5 

27-3 

6.2 

67.4 

5-1           27.5 

" 

68.1 

23-9 

8.0 

68.5 

6.0           25.5 

tt 

68.3 

23.1 

8.6 

68.3 

6.7           25.0 

36 

.  .  . 

.  .  . 

66.6 

4.1           29.3 

tt 

57-7 

38.4 

3-9 

n 

65.0 

28.3 

6.7 

68.8 

5-9          25.3 

tt 

68.1 

21  .2 

10.7 

68.9 

9.4          21.7 

45 

61.8 

32-9 

5-3 

.  .  . 

...             ... 

tt 

65.8 

25-3 

8.9 

68.4 

8.8          22.8 

" 

66.0 

24-0 

IO-O 

68.6 

10.  i           21.3 

3i5  SODIUM    SULPHATE 

SOLUBILITY  OF  SODIUM  SULPHATE  IN  AQUEOUS  PROPYL  ALCOHOL 

AT  20°. 

(Linebarger  —  Am.  Ch.  J.  14,  380,  '92.) 


Gms.  CgHyOH 

Gms.  Na2SO4 

Gms.  C3H7OH 

Gms.  Na2S 

per  ioo  Gms. 
Alcohol-Water 

per  ioo 
Gms.  Sat. 

per  ioo  Gms. 
Alcohol-Water 

per  ioo 
Gms.  Sat. 

Mixture. 

Solution. 

Mixture. 

Solution. 

42.20 

1.09 

56-57 

o-55 

49-77 

I  .15 

60.64 

0.44 

55-65 

0.72 

62.81 

0.38 

ioo  gms.   H2O   dissolve   183.7   gms.   sugar  +  30.5   gms.   Na2SO4  at 
31.25°,  or  ioo  gms.  sat.  solution  contain  52.2  gms.  sugar  +  9.6  gms. 

Na2SO4.  (Kohler  — Z.  Ver.  Zuckerind.  47,  447,  '97.) 

SODIUM  (Bi)  SULPHATE  NaHSO4. 

ioo  gms.  H2O  dissolve  28.6  gms.  at  25°,  and  50.0  gms.  at  100°. 

ioo  gms.  alcohol  dissolve  1.4  gms.  at  25°.  <U.  s.  p.) 

SODIUM    THIO    SULPHATE   Na2S2O3. 

SOLUBILITY  IN  WATER. 

(Young  and  Burke  —  J.  Am.  Chem.  Soc.  26,  1417,  '04.) 


Gms.  Na2S203  per 

Gms.  Na2S2O3  per 

t  o                       ioo  Gms.                             So»d               t  o 

IOO 

Gms. 

Solid 

PVi<*c?A 

Solution. 

WaterT 

Solution. 

Water. 

.rnase. 

IO 

37.38 

59*69   Pentahydrate  (com.V 

20 

62  .11 

163.92 

Monohydrate 

2O 

41  .20 

70.07 

25 

62.73 

168.32 

» 

25 

43-15 

75-90 

30 

63  -53 

174-20 

" 

30 

45-19 

82.45 

20 

55-15 

122.68 

Dihydrate 

35 

47-71 

91.24 

25 

56-03 

127-43 

" 

40 

50.83 

103-37 

30 

57-13 

133  .27 

" 

45 

55-33 

123.87 

35 

58-13 

138.84 

it 

20 

49-38 

97.55      Pentahydrate  (8) 

40 

59-17 

144.92 

" 

25 

52-15 

108.98 

5° 

62.28 

165.11 

•• 

28 

54-48 

119-69 

33-5 

58.59 

141.48 

Tetrahydrate  (?) 

29-5 

55  -85 

126.50 

36-2 

60.51 

153-23 

» 

30 

56.57 

130.26 

36-6 

62.80 

168.82 

" 

ioo  gms.  alcohol  dissolve  0.0025  gm.  Na2S2O3  and  0.0034  gm. 
Na2S2O3.5H2O  at  room  temperature.  (Bodtker  —  z.  physik.  Chem.  22, 510,  '97.) 

ioo  gms.  alcohol  of  0.941  Sp.  Gr.  dissolve  33.3  gms.  at  15.5°. 

(See  also  Parmentier  —  Compt.  rend.  122,  136,  '96.) 

SODIUM  SULPHITE   Na2SO8. 

ioo  gms.  H2O  dissolve   14.1   gms.  at  o°,  25.8-28.7  gms.  at  20°,  and 

49.5  gms.  at  40°.  (Kremers  —  Pogg.  Ann.  99,  50,  '56.) 

SODIUM    TELLURIATE    Na2TeO4.2H2O. 

ioo  gms.  H2O  dissolve  0.77  gm.  Na2TeO4  at  18°,  and  2.0  gms.  at 
100°.  Solid  phase  Na2TeO4.2H2O. 

ioo  gms.  H2O  dissolve  1.43  gms.  Na3TeO4  at  18°,  and  2.5  gms.  at  50°. 
Solid  phase  Na2TeO4.4H2O.  (Myiius  —  Ber.  34. 2208,  '01.) 


SODIUM   TUNGSTATE  316 

SODIUM    TUNGSTATE     (Wolframate)    Na2WO4.2H3O. 
SOLUBILITY  IN  WATER. 

(Funk  —  Ber.  33,  3701,  'oo.) 
Mols.  pm=  Mols. 


t.     Naper        a4  Solid  Na2WO4  per 

*  '       100  Cms.  V  Phase.  t   '       100  Gms.  i-  Phase. 


Solution.       **>os.  Solution. 

—  5         30.60  2.70      Na2WO4.ioH2O   —  3.5      41.67  4.37       Na2WO4,2H2O 

-4      31.87         2.86  "  +5         41-73         4-39 

~3-5  32-98        3-01  18        42-0          4-40 

-2          34.52  3.23  21  42.27  4.48 

o      36-54        3-52  43-5     43'98         4-8i 

+  3      39-20        3.95  "  80.5     47-65        5-57 

5      41.02        4.26  100        49.31         5.95 

Sp.  Gr.  of  sat.  solution  at  18°  =  1.573.    For  Sp.  Gr.  determinations 
of  aqueous  solutions  at  20°,  see  Pawlewski  —  Ber.  33,  1223,  'oo. 

SODIUM    Fluo    ZIRCONATE     5NaF.ZrF4. 

100  gms.  H2O  dissolve  0.387  gm.  at  18°,  and  1.67  gms.  at  100°. 

(Marignac  —  J.  pr.  Chem.  83,  202,  *6i.) 

STRONTIUM    BENZOATE   Sr(C7H6O2)2.H2O. 
SOLUBILITY  IN  WATER. 

(Paietta  —  Gazz.  chim.  ital  36,  II,  67,  '06.) 
t°  15-7°       24.7°     31.4°      40.9° 

Gms.  Sr  (C7H5O2)2  per  100  gms.  solution       5  .31       5.4       5  .56       5  .77 

STRONTIUM    BROMATE    Sr(BrO3)2. 

One  liter  of  aqueous  solution  contains  0.9  gram  molecules  or  309 

gms.  Sr(BrO3)2  at  l8°.  (Kohlrausch  —  Sitzb.  K.  Akad.  Wiss.  (Berlin)  90,  '97.) 

STRONTIUM    BROMIDE    SrBr2.6H2O. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  results  of  Kremers  —  Pogg.  Ann.  103,  65,  '58;  and  Etard  —  Ann.  chim. 
phys.  [7]  2,  540,  '94.) 

to  Gms.  SrBr2  per  100  Gms.  t<j  Gms.  SrBr2  per  TOO  Gms. 

Solution.  Water.  Solution.  Water. 

o  46-0  85.2  40  55-2  I23-2 

10  48-3  93-o  5°  57  -6  W-8 

20  50-6  102.4  60  60.0  150-0 

25  51.7  107.0  80  64.5  181.8 

30  52.8  111.9  100  69.0  222.5 

Sp.  Gr.  of  sat.  solution  at  20°  approximately  1.70. 

100  gms.  abs.  alcohol   dissolve  64.5    gms.  SrBr2  at  o°.     Sp.  Gr.  of 

Solution  =  1  .  2  1  .  (Fonzes  ;  Diacon  —  J.  pharm.  chim.  [6]  I,  59,  '95-) 

STRONTIUM    CARBONATE    SrCO3. 

One  liter  of  water  dissolves  0.0082  gm.  at   8.8°    and  0.0109  gm. 
at  24°  by  conductivity  method. 

(Holleman  —  Z.  physik.  Chem.  12,  130,  '93;  Kohlrausch  and  Rose  —  Ibia.  12,  241,  '93.) 

One  liter  of  water  saturated  with  CO2  dissolves  1,19  gms.  Sr(HCO3)2. 


317     STRONTIUM  CHLORATE 
STRONTIUM  CHLORATE  Sr  (CIO,),. 

100  gms.  H2O  dissolve  174.9  gms.  Sr(ClO)2,  or  100  gms.  sat.  solution 
contain  63.6  gms.  at  18°.     Sp.  Gr.  of  solution  is  1.839. 

(Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 


STRONTIUM    CHLORIDE   SrCl2.6H2O. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  the  results  of  Mulder;  Etard;  see  also  Tilden  —  J.  Chem.  Soc.  45,  409,  '84.) 


t<>         Gms.  SrCl2  per  ioo  Gms.        Solid 

Solution 

Water.              Phase. 

—  2O            26.O 

35-1         SrCl2.6H2O 

60 

o         30-3 

43-5 

70 

10         32.3 

47-7 

80 

20            34.6 

52.9 

IOO 

25        35-8 

55-8 

120 

30        37-o 

58-7 

I4O 

40        39-5 

65-3 

1  60 

50        42.0 

72.4 

1  80 

Transition 

temperature  about 

62.5°. 

=  1.334;  at  15°  =  1.36. 

Gms.  SrCl2  per  100  Gms. 


Solution. 

Water 

60 

45-o 

8l.8 

70 

46.2 

85  -9 

80 

47-5 

9o-5 

IOO 

50.2 

100.8 

120 

53-o 

112.  8 

I4O 

55-6 

125  .2 

1  60 

58-5 

I4I.O 

1  80 

62  .0 

163.1 

Solid 
Phase. 

SrCl2.6H20 


Sp.  Gr.  of  sat.  solution  at  o° 


SOLUBILITY  OF  STRONTIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROCHLORIC  ACID  AT  o°. 

(Engel  —  Ann.  chim.  phys.  [6]  13,  376,  '88.) 


Mg.  Mols.  per 

10  cc.  Solution. 

51  .6 

44-8 

HC1. 
O 

6.1 

37-85 

12.75 

27.2 

22  .O 

23-3 
28.38 

14.0 

37-25 

4-25 

52-75 

Sp.  Gr.  of 

Solution. 

•334 
•3°4 
.269 
.220 
.201 

.167 


Grams  per  ioo  cc.  Solution. 


SrCl2. 
40-9 

35-5 
30-0 

21  .56 
17.44 
II  .09 

3-37 


HCl. 
O.O 
2  .22 
4-65 

8-49 
!o.35 

13-58 

19.23 


100  gms.  abs.  methyl  alcohol  dissolve  63.3  gms.  SrCl2.6H2O  at  6°. 
100  gms.  abs.  ethyl  alcohol  dissolve  3.8  gms.  SrQ2.6H2O  at  6°. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  787,  '93.) 


SOLUBILITY  OF  STRONTIUM  CHLORIDE  IN  AQUEOUS  ETHYL 
ALCOHOL  SOLUTIONS  AT  18°. 

(Gerardin  —  Ann.  chim.  phys.  [4]  5,  156,  '65.) 


Sp.  Gr,  of 
Aq.  Alcohol 
ato°. 

Wt. 

per  cent 
Alcohol. 

Gms.  SrCl2 
per  loo  Gms. 
Alcohol. 

Sp.  Gr.  of 
Aq.  Alcohol 
ato°. 

Wt. 
per  cent 
Alcohol. 

Gms.  SrClj 
per  too  Gms. 
Alcohol. 

O.QQO 

6 

49-8l 

o-939 

45 

26.8 

0.985   - 

10 

47-0 

0.909 

59 

19.2 

o-973 

23 

39-6 

0-846 

86 

4-9 

0.966 

30 

35-9 

0.832 

9* 

3-2 

o-953 

38 

3°-4 

STRONTIUM    CHROMATE          318 

STRONTIUM    CHROMATE    SrCrO4. 

SOLUBILITY  IN  WATER,  ETC.,  AT  15°. 

(Fresenius  —  Z.  anal.  Chem.  29,  419,  '90;  30,  672,  '91.) 

Cms.  SrCrO4  Cms.  SrCrO4 

Solvent.  per  i  oo  Solvent.  per  100 

Gms.  Solvent.  Gms.  Solvent. 

Water  0.12          Aq.  Ethyl  Alcohol  (29%)        0-0132 

Aq.  NH4C1  (5  %)  o .  195         Aq.  Ethyl  Alcohol  (53  %)         o  .002 

Aq.  CH3COOH(i%)      1.57 

STRONTIUM    FLUORIDE    SrF2. 

One  liter  of  water  dissolves  1.87  rng.  equiv.  or  0.117  gm.  SrF2  at 

l8°,  by  conductivity  method.  (Kohlrausch  —  Z.  physik.  Chem.  50,  356,  '04-05-) 

STRONTIUM    HYDROXIDE   Sr(OH)2. 

SOLUBILITY  IN  WATER. 

(Scheibler  —  N.  Z.  Rubenzuckerind.  7,  257  ;  abstract  in  J.  pharm.  chim.  [5]  8,  540,  '83.) 
Grams  per  looprams  Solution.  Grams  per  TOO  cc.  Solution. 

SrO.  Sr(OH)2.8H2O."  SrO.  Sr(OH)2.8H2O.  " 

o  0.35  0.90  0.35  0.90 

10  0.48  1.23  0.48  1.23 

20  0.68  i-74  0.68  i-74 

30  i. oo  2.57  i. 01  2.59 

40  1.48  3.80  1.51  3.87 

50  2.13  5.46  2.18  5.59 

60  3.03  7.77  3.12  8.00 

70  4-35  IX-16  4-55  XI-67 

80  6.56  16.83  7-°2  18.01 

90  12.0  30-78  i3-64  34-99 

100  18.6  47-71  22.85  58-61 

STRONTIUM    IODATE    Sr(IO3)2. 

100   gms.  H2O   dissolve    0.026  gm.  at    15°,   and   0.72-0.91    gm.  at 

IOO   .  (Gay-Lussac;  Rammelsberg  —  Pogg.  Ann.  44,  575,  '38.) 

STRONTIUM    IODIDE   SrI2.6H2O. 

SOLUBILITY  IN  WATER. 

(Average  curve  from  the  results  of  Kremers  —  Pogg.  Ann.  103, 65,  '58;  and  Etard  —  Ann.  chim.  phys. 

[?]  2,  528,  '74-) 

Gms.  SrI2  per  100  Gms            Solid                        to  Gms.  SrI2  per  100  Gms.           Solid 

Solution.           Water.             Phase.  Solution.           Water.            Phase. 

O            62.3            165.3        SrI2.6H2O                  90  78.5            365-2      SrI2.2H2O 

20           64.0            177.8               "                       IOO  79.3            383.1 

40            65.7             I9I-5                "                        120  80.7            4l8.I 

60         68.5         217.5  "  I4°         82.5         471-5 

80         73.0         270.4  "  175         85.6         594-4 

Transition  temperature  about  90°.  Sp.  Gr.  of  sat.  solution  at  20°  =• 
2.15. 

loo  gms.  saturated  solution  of  strontium  iodide  in  absolute  alcohol 
contain  2.6  gms.  SrI2  at  — 20,  3.1  gms.  at  +  4°,  4.3  gms.  at  39°,  and  4.7 

gms.  at  82°.  (Etard.) 


319  STRONTIUM    MALATB 


STRONTIUM    MALATE   SrC4H4O6. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Basadonna  —  Bull.  soc.  chim.  35,  731,  '06.) 


0 

Gms.  per  100 

Gms.  per  100 

0 

Gms.  per  100 

* 

cc.  Solution. 

. 

cc.  Solution. 

*  • 

cc.  Solution. 

20 

0.448 

40 

I-385 

55 

2.460 

25 

0-550 

45 

1-743 

60 

2.821 

30 

0.752 

5° 

2.098 

65 

3.148 

35 

1.036 

3.360 

STRONTIUM    MOLYBDATE   SrMoO4. 

100  gms.  H2O  dissolve  0.0104  gm.  SrMoO4  at  17°. 

(Smith  and  Bradbury  —  Ber.  24,  2930,  '91.) 

STRONTIUM    NITRATE   Sr(NO3)2. 

SOLUBILITY  IN  WATER. 

(Mulder;  see  also  Etard  for  slightly  lower  results.) 

-o       Gms.  Sr(NO3)2  per  100  Gms.         Solid  to    Gms.  Sr(NO3)7  per  100  Gms.      Solid 

'  Solution.  Water.  Phase.  Solution.         Water.  Phase. 

O  28.3  39.5  Sr(N03)2.4H20  40  47.7  91.3          Sr(N03)« 

10  35-5  54-9  5°  48 -i  92.6 

20  41.5  70.8  60  48.5  94.0 

25  44.1  79.0  80  49.3  97.2 

30  46.7  87.6  "       100  50.3  loi.i 

Transition  temperature  about  31°.    Sp.  Gr.  of  sat.  solution  at  20°  = 
1.44. 

100  gms.  absolute  alcohol  dissolve  0.024  gm.  Sr(NO3)2. 
100  gms.  rectified  spirit  dissolve  0.50  gm.  Sr(NO3)2. 

(Hill  — Pharm.  J.  Trans.  [3]  19,  420,  '88.) 

STRONTIUM    OXALATE   SrC2O4.H2O. 

One  liter  of  aqueous  solution  contains  0.52  mg.  equivalent  SrC2O4 
or  0.046  gm.  at  18°,  conductivity  method. 

(Kohlrausch  —  Z.  physik.  Chem.  50,  356,  '04- '05.) 

SOLUBILITY  OF  STRONTIUM  OXALATE  IN  AQUEOUS  ACETIC  ACID 
SOLUTIONS  AT  26°-27°. 

(Herz  and  Muhs  —  Ber,  36,  3715,  '03.) 


Normality 

Gms.  per  100  cc.  Solution. 

Normality 

Gms.  per  100  cc.  Solution. 

of 
Acetic  Acid. 

CHsCOOH. 

Residue 
SrC204.H20. 

of 
Acetic  Acid. 

CKaCOOH. 

Residue 
SrC2O4.H2O. 

o.o 

O-O 

0.009 

3.86 

23.16 

0-0898 

0.58 

3-48 

0.0526 

5-79 

34-74 

0.0496 

i-45 

8.70 

O.O622 

16.26 

97-56 

o  .  0060 

2.89 

J7-34 

0-0642 

STRONTIUM    SALICYLATE    Sr(C6H4OH.COO)2.2H2O. 

100  gms.  H2O  dissolve  5.55  gms.  at  25°,  and  28.6  gms.  at  b.  pt. 

(u.  s.  P.) 

100  cc.  aqueous  solution  contain  1.830  gms.  anhydrous  salt.      (Banhe.) 
100  gms.  alcohol  dissolve  1.5  gms.  at  25°,  and  9.52  gms.  at  b.  pt. 

(U.  S.  P. ;  Barthe  —  Bull.  soc.  chim.  [3]  u,  519,  '94.) 


STRONTIUM    SULPHATE  320 

STRONTIUM    SULPHATE   SrSO4. 

One  liter  of  aqueous  solution  contains  1.24  mg.  equivalents  or  0.114 
gm.  SrSO4  at  18°,  by  conductivity  method. 

(Kohlrausch  —  Z.  physik.  Chem.  50,  356,  '04- '05;  Holleman  —  Ibid.  12,  129,  '93;  Wolfmann  —  Oster. 
Ung.  Z.  Zuckerind.  25,  997,  '97.) 

SOLUBILITY  OF  STRONTIUM  SULPHATE  IN  AQUEOUS  SOLUTIONS    OF 
HYDROCHLORIC,  NITRIC,  CHLORACETIC  AND  FORMIC  ACIDS. 

(Banthisch  —  J.  pr.  Chem.  [2]  29,  52,  '84.) 


cc.  of  Aq. 
Acid    con- 

In Aq.  HC1 
Gms.  per  100  cc. 

In  Aq.  HNO3 
Gms.  per  100  cc. 

In  Aq.  CH2C1COOH     In  Aq.  HCOOH 
Gms.  per  100  cc.  Sol.     Gms.  per  100  cc. 

taining    i 
Mg.  Equr 
in  each  caa 

so 

so 

I. 

'  CH2C1 
COOH. 

>!  '  HC1. 

SrS04. 

HNO3. 

SrS04. 

SrSO4.     HCOOH. 

SrS04. 

0.2 

18. 

23 

0.161 

31 

•S2 

0 

.381 

...             ... 

.  .  . 

0.5 

>j 

.29 

0.207 

12 

-6l 

0 

•307 

...             ... 

.  .  . 

I  .0 

3 

65 

0.188 

6 

•30 

0 

.217 

94 

•47 

O.O26      46.02 

O.O24 

2  .O 

j 

.82 

0.126 

3 

0 

.138 

47 

•23 

O.O22 

10.  0 

o. 

36 

0.048 

o 

•63 

0 

•049 

... 

SOLUBILITY  OF  STRONTIUM  SULPHATE  IN  SULPHURIC  ACID 
SOLUTIONS. 

r,  f  Gms.  SrSO4 

t°.  HCO  I**100  Authority. 

H2SO<-  Gms.  Acid. 

Ord.        Concentrated  5  . 68      (Struve  —  Z.  anal.  Chem.  9,  34,  1870.) 

"        fuming  9.77 

91  %  O  .08      (Varenne  and  Paulean  —  Compt.  rend.  93,  1016,  ?8i.) 

70      Sp.  Gr.  1 .843  =  99  °/0  14-0  (Garside  —  Chem.  News,  31,  245,  '75.) 

SOLUBILITY  OF  STRONTIUM  SULPHATE  IN  AQUEOUS  SALT 
SOLUTIONS. 

(Virck  — Chem.  Centralb.  402,  '62.) 
In  Aq.  NaCl.  In  Aq.  KC1.  In  Aq.  MgCl2.  In  Aq.  CaCl2. 


(a.)                (b.) 
8.44      0.165 
15.54      0.219 
22.17      0-lSl 

(a.)                (b.) 
8.22       0.193 
12-54      0.193 

18.08    0.251 

(«.)          (&.)' 
1.59    0.199 
4.03     0.206 
13.63     0.242 

(a.)                 (b.) 
8.67       0.176 
16.51       0.185 
33.70      O.I7I 

(a)  =  Gms.  salt  per  100  gms.  aq.  solution.     (6)  =  Gms.  SrSO4  per 
100  gms.  solvent. 


STRONTIUM    TARTRATE  SrC4H4O6.3H2O. 
SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder  —  Bull.  soc.  chim.  [3]  33,  751,  '05.) 


t«. 

Gms. 
SrC4H406 
.3H20  per 

100  CC. 

t<>. 

Gms. 
SrC<H4O6 
.3H20  per 

100  CC. 

t<>. 

Gms: 
per  100  cc. 

Solution. 

Solution. 

Solution. 

0 

O.II2 

25 

0.224 

60 

0.480 

10 

0.149 

30 

0.252 

70 

0.580 

15 

0.174 

40 

0-328 

80 

0.680 

20 

0.200 

50 

0.407 

85 

o-755 

:H3COOH. 

SrC4H4O0.3H26. 

Acetic  Acid. 

CH3COOH. 

SrC4H4O6.3H2C 

o.o 

O.227 

3-77 

21.85 

I  .051 

3-39 

0.678 

5-65 

33-90 

0.982 

8.15 

0.864 

16.89 

101.34 

0.184 

17  .10 

0.996 

321  STRONTIUM    TARTRATE 

SOLUBILITY  OF  STRONTIUM  TARTRATE  IN  AQUEOUS  SOLUTIONS  OF 
ACETIC  ACID  AT  26°-27°. 

(Herz  and  Muhs  —  Ber.  36,  3715,  '03.) 

Gms.  per  ioo  cc.  Solution. 

kid.     CH3COOH.     SrC4H4O0.3H26.          Acetic  Acid."      c 
0-0 

1.425 


STRONTIUM    (Di)    TUNGSTATE    SrW2O7.3H2O. 
100  cc.  H2O  dissolve  0.35  gm.  at  15°. 

(Lefort  —  Ann.  chim.  phys.  [5]  15,  326,  '78.) 

STRYCHNINE   C21H22N2O2. 

SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(U.  S.  P.;  at  20°,  Muller  —  Apoth.-Ztg.  18    258,  '03;  Schindelmeiser.) 

Gms.  C21H22N2O2  Gms.  C2  H22N2O2 

per  100  Gms.  per  100  Gms. 

Solvent.  < — r~ " •  Solvent.  . — • 

Solution         Solvent  Solution      Solvent 

at  20°.          at  25°.  at  20*.       at  25°. 

Water  0.021  0.016     Petroleum  Ether  0.0093 

Water  Sat.  with  Ether  0.0166        ...       Acetic  Ether  0.1972       ... 

Ether  0.0432  0.0182   Carbon  Tetra  Chloride  0.158    o.645(i7°)(S.) 

Ether  Sat.  with  H2O  0.0513        ...       Alcohol  ...       0.909 

Benzene  o.  770  o.  666     Amyl  Alcohol  ...       o.  555 

Chloroform  100+  16. 6         Glycerine  ...       0.25   (15°) 

ioo  gms.  pyridine  dissolve  1.24  gm.  C21H22N2O2  at  26°. 

(Holty  —  J.  Physic.  Chem.  9,  764,  '05.) 

SOLUBILITY  OF  STRYCHNINE  NITRATE  AND  SULPHATE  IN  SEVERAL 

SOLVENTS. 

(U.  S.P.) 

Strychnine  Nitrate.  Strychnine  Sulphate. 

Gms.  per  TOO  Gms.  Solvent  at:  Gms.  per  ioo  Gms.  Solvent  at: 

Solvent.  ' * 7-3 >  < 3 " r~s » 

25  .  80  .  25  .  80  . 

Water  2.38  12.5  3.23  16.6 

Alcohol  o .  83  i .  66  (60°)  1.54  5-o  (60°) 

Chloroform  0.64  0.31 

Glycerine  1.66  4-0(15°)  22.5(15°) 


SUBERIC    ACID    CeH12(COOH)2. 

SOLUBILITY  IN  WATER. 

(Lamouroux  —  Compt.  rend.  128,  998,  '99.) 
t°.  o°.  15°.  20°.  35°.  S°r-  65° 

Gms.  C6H12(COOH)2 

per  ioo  cc.  solution     0.08        0.13        0.16        0.45        0.98        2.22 


SUCCINIC    ACID  322 

SUCCINIC    ACID  (CH2)2(COOH)2. 

SOLUBILITY  IN  WATER. 

(Miczynski  —  Monatsh.  Chem.  7,  263,  '86;  Van  der  Stadt  —  Z.  physik.  Chem.  41,  355,  '02;  Lamouroux 
—  Compt.  rend.  128,  998,  '99;  for  other  concordant  results,  see  Bourgoin  —  Bull.  soc.  chim.  [2]  21,  no 
'74;  Henry  —  Compt.  rend.  99.  H57»  '84.) 

Gms.  Succinic 

o  Gms.  (CH2)2(COOH)2  per  100     /r™^p^oO  Mol.  per  cent. 

'Gms.  H20.         cc.  Solution."      (      2)^r  H2O.          (CH2)2COCOO". 

100  Gms.  H2O. 

o        2.80    2-78(L.)    2.34    99-58     0.42 
10        4-51     4-o        3-80    99-32     0.68 

20  6.89      5.8  5.77       98.97        1.03 

25  8.06       7-0  6.74      98.80        1.20 

30  10.58  8.5  8.79  98.44             1-56 

40  16.21  12.5  13.42  97-64            2.36 

50  24.42  18.0  19.95  96-53            3-47 

60  35.83  24.5  28.77  95-07            4-93 

70  51-07  40.11  93-26            6.74 

80  70-79  54-oS  91.12            8.88 

89.4  95-45  •••  70.62  88.71  11.29 

104-8  146.3  ...  101.2  84.57  15.43 

115.1  188.5  ...  126.8  81.4  18.6 

134-2  335-4  187-8  74-72  25.28 

159-5  748.2  ...  295.2  65.27  34.73 

180.6  1839-0  ...  408.5  57.6  42.4 

182.8  oo  ...  542-3  50-0  50-0 

174.4  808.5  40.7  59.3 

153.3  ...  2239.0  19.86  80.14 

128.0  ...      ...  8865.0     5.89  94.11 

118.8-119  •••                •••  °°                   o-oo  100.00 

SOLUBILITY  OF  SUCCINIC  ACID  IN  ALCOHOLS  AND  IN  ETHER. 

(Timofeiew  —  Compt.  rend.  112,  1137,  '91;  at  15°,  Bourgoin  —  Ann.  chim.  phys.  [5]  13,  405,  '78.) 

Gms.  (CH2)2(COOH)2  per  100  Gms. 

Solvent.  t Solvfnt  at: 

-i°.  +i5°-  +21.5°. 

Abs.  Methyl  Alcohol  10.51                                    19 . 40 

Abs.  Ethyl  5 .06            I2-59                9-49 

90%      "  7-51 

Abs.  Propyl       "  2.11                ...                   4-79 

Abs.  Ether  1.265 

DISTRIBUTION  OF  SUCCINIC  ACID  BETWEEN  WATER  AND  AMYL 
ALCOHOL  AT  20°. 

(Herz  and  Fischer  —  Ber.  37,  4748,  '04.) 

Millimols  £C4H6O4  Gms.  C4HeO4  per  Millimols  $C4H6O4  Gms.  C4H6O4 

per  10  cc.  loo  cc.  per  10  cc.  per  100  cc. 


Alcohol 

Aq.                 Alcohol 

Aq. 

Alcohol 

Aa. 

Alcohol 

Aq.  " 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

Layer. 

0.1888 

O 

.2684 

O 

.1114 

0-1584 

3 

.899 

6 

•0795 

2.302 

3.588 

0.3643 

0 

•5252 

O 

.215 

0-310 

5 

.199 

8 

•099 

3.069 

4-779 

0.7077 

I 

•0373 

0 

.418 

0.612 

6 

•334 

10 

.170 

3-739 

6.000 

1-440 

2 

.1266 

0 

.850 

J-255 

7 

.119 

ii 

•555 

4.202 

6.821 

2.7I5 

4 

•0495 

I 

.603 

2.391 

323  SUCCINIC    ACI1S 

SOLUBILITY  OF  SUCCINIC  ACID  IN  AQUEOUS  ACETONE  AT  20°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  41,  320,  '04.) 

cc.  Acetone  per     C4H6O4  per  ioo  cc.  Solution.  cc.  Acetone  per        C4H6O4  per  ioo  cc.  Solution 

100  cc.  Solution.    Millimols.  Grams.  '  100  cc.  Solution.          Millimols.  Grams.     ' 

o  107.8  6.363  60  275.7  16.27 
Jo  127.4  7-5*9  7o  278.5  16.44 
20  155.8  9  J94  80  265.3  15.66 

30        186.7       11-02  90          201-9       11.91 

40  225.4          13-30  ioo  51.5  3.04 

50         254.3        15.01 

SOLUBILITY  OF  SUCCINIC  ACID  IN  AQUEOUS  GLYCERINE 
SOLUTIONS  AT  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  45,  268,  '05.) 


Wt.% 
Glycerine 

CaHeO-i  per  ioo  cc. 
Solution. 

Sp.  Gr. 
of 

Wt.% 
Glycerine 

C4HeO4  per  ioo  cc. 
Solution. 

Sp.  Gr. 
of 

in  Solvent 

•  Millimols. 

Grams. 

Solutions. 

in  Solvent. 

Millimols. 

Grams. 

Solutions. 

O 

133-4 

7 

.874 

I 

.0213 

40 

•95 

105.8 

6.244 

I 

.  II2Q 

7-15 

128.2 

7 

.566 

I 

-0407 

48 

.70 

99-9 

5  -896 

I 

.I208 

20-44 

II8-3 

6 

.982 

I 

-0644 

69 

.20 

88-5 

5-223 

I 

.1804 

3I-55 

109.7 

6 

.476 

I 

.0897 

IOO 

.00* 

74.6 

4.440 

I 

•2530 

*  Sp.  Gr.  of  Glycerine—  i -2555.     Impurity  about  i  .5  per  cent. 

SUCCINIMID  C2H4<£°>NH. 

SOLUBILITY  IN  WATER  AND  IN  ETHYL  ALCOHOL. 
Interpolated  from  original  results.  (SpeyerS  -  Am.  j.  sd.  [4]  14, 294,  '02:, 

In  Water.  In  Ethyl  Alcohol. 

t°.         Wt.  of  T  cc.         Mols.  per        Gms.  per  ioo  Wt.oficc.     Mols.penoo      Gms.   per  10 

Solution.       ioo  Mols.  H2O.     Gms.  H2O.  Solution.    Mols. C2H5OH.  Gms. C2H6OH 

o    1.025     1.58     8.69      0.815     0.88     1.89 
10     .035    2.4     14.0       0.809    1.35    2.7 

2O       .052       4-O        23-0          O.8o6      2-OO      4-1 
25       -067       5-9        33-0          0-805       2-5        5.3 

30  .086  8.0  45.0  ;    0.804  3.1  6.8 

40  .120  12.8  70.0  0.809  4.9  10.5 

50  .145  17.8  96.0  0.816  7.8  16.0 

60  .167  22.6  124.0  0-835  12.3  26.5 

70  .189  27.5  152-0  0.873 

80  .204  32.8  0.954 

SUCCINIC    NITRIL  (Ethylene  Cyanide)    CNCH2CH2CN. 

The  solubility  of  succinic  nitril  in  water  and  also  in  aqueous  sodium 
chloride  solutions  at  various  temperatures  has  been  determined  by 
Schreinemaker  (Z.  physik.  Chem.  23,  439,  '97),  and  the  results 
presented  in  terms  of  mols.  of  nitril  per  ioo  mols.  of  nitril  +  H2O. 
The  following  calculation  of  these  results  to  gram  quantities  was 

made  by  Rothmund.  (Landolt  and  Bornstein,  3d  ed.  p.  59^,  '06.) 

Gms.  CNCH2CH2CN  per  ioo  Gms.  Gms.  CNCH2  CH2CN  per  ioo  Gms. 

t°.  t s  t°.         , % 

Aq.  Layer.     Nitril  Layer.  Aq.  Layer.       Nitril  Layer. 

18.5  10.2  92.0  53-5  33-2  66.4 

20  ii. o          91-5  55  40-3  62.8 

39  85 .2  55 .4  (crit.  temp.)  51.0 

45  22.0 


SUGAR  324 

SUGAR  C12H22On   (Cane  Sugar.) 

SOLUBILITY  IN  WATER. 

(Herzfeld  —  Z.  Ver.  Zuckerind.  181,  '92;  see  also  Courtonne  —  Ann.  chim.  phys.  [5]  12,  569,  '77.) 


Gms.  Ci2H22On  per  t*.  Gms. 

ioo  Gms.  ioo  Gms. 


Solution.  Water.  Solution.  Water. 

o     64.18  179-2  40  70.42  238.1 

5     64.87  184.7  45  7J-32  248.7 

10     65.58  I9°-5  5°  72-25  260.4 

15     66.33  !97-o  60  74-18  287.3 

20     67.09  203.9  7°  76.22  320.4 

25     67.89  211.4  80  78-36  362.1 

30     68.70  219.5  90  80. 61  4*5-7 

35     69.55  228.4  ioo  82.97  487.2 

6p.  Gr.  of  sat.  solution  at  15°  =  1.329;  at  25°  =  1.340. 


SOLUBILITY  OF  SUGAR  IN  AQUEOUS  SALT  SOLUTIONS  AT  30°,  50°. 

AND   '70°' 

Interpolated  from  original  results. 

(Schukow  —  Z.  Ver.  Zuckerind.  50,  313,  'oo.) 
Gms.  Ci2H22Oa  per  ioo  grams  H2O  in  Aq.  Solution  of: 


*•    . 

unis.  oau  per 
ioo  Gms.  H2O. 

KC1. 

KBr. 

KNO3. 

NaCl. 

CaCl2. 

30 

O 

219.5 

219.5 

219.5 

219.5 

219.5 

10 

216 

218 

217 

210 

I97 

tt 

20 

221 

22O 

216 

211 

189 

ft 

30 

228 

224 

216 

219 

192 

" 

40 

237 

228 

217 

233 

2OO 

" 

50 

218 

250 

2X3 

tt 

60 

269 

243 

50 

O 

260.4 

260.4 

260.4 

260.4 

260.4 

tt 

IO 

261 

262 

260 

255 

239 

It 

20 

266 

266 

261 

260 

228 

li 

30 

274 

272 

262 

269 

228 

tt 

40 

284 

276 

262 

284 

236 

it 

50 

296 

280 

263 

302 

253 

tl 

60 

276 

10 

O 

320.5 

320.5 

320.5 

320.5 

320.5 

*t 

IO 

326 

324 

321 

323 

295 

•• 

20 

334 

328 

324 

330 

286 

(i 

30 

345 

334 

327 

344 

286 

ti 

40 

357 

34i 

331 

361 

295 

tt 

50 

370 

349 

334 

384 

308 

tt 

60 

384 

357 

337 

406 

327 

325 


SUGAR 


SOLUBILITY  OF  CANE  SUGAR  IN  SATURATED  AQUEOUS  SALT 
SOLUTIONS  AT  31.25°. 

(Kohler  — Z.  Ver.  Zuckerind.  47,  447,  '97.) 


Gms.  Sugar  per  100  Gms. 


Salt. 

CH3COOK 

C3H7COOK 

C3H4.OH.(COOK)3 

K2C03 

KC1 

CH3COONa 

NaCl 


SOLUBILITY  OF  CANE  SUGAR  IN 

(Scheibler  —  Ber.  5,  343,  '72; 

Results  at  o°. 


Gms.  Sugar  per  icoGms- 


Solution. 

Water. 

oaii. 

Solution. 

Water. 

324-8 

Na2C03 

64.73 

229.2 

49.19 

306.1 

KNO3 

61.36 

224.7 

50-30 

303-9 

K2S04 

66.74 

219.0 

56.0 

265.4 

CH3COOCa 

60.  12 

190.0 

62.28 

246.5 

Na2SO4 

52.20 

183-7 

59-93 

237.6 

CaCl2 

42.84 

I35-I 

62  .17 

236-3 

MgS04 

46-52 

119.6 

AQUEOUS  ALCOHOL  SOLUTIONS. 

correction  Ber.  24,  434,  '91.) 

Results  at  14°.  Results 


Per  cent 
Alcohol 

Sp.  Gr. 
of  Solution 

Gms.  Sugar 
per  100  cc. 

Sp.  Gr. 

of  Solution 

Gms. 

per  100  cc.  Solution. 

-    T' 

Gms.  Su 

by  Vol. 

at  17.5°. 

Solution. 

at  17.5°. 

Sugar. 

C2H6OH. 

H20.' 

per  TOO 
Solutio 

0 

I-325 

85.8 

1.326 

87-5 

O 

45-10 

10 

1.299 

80-7 

1.300 

8l.5 

3-91 

44.82 

95-4 

20 

1.236 

74-2 

1.266 

74-5 

8.52 

43-83 

90.0 

30 

1.229 

65-5 

1-233 

67.9 

*3-74 

41.87 

82.2 

40 

I.I82 

56.7 

I.I85 

58.0 

20.24 

40.38 

74-9 

50 

I  .129 

45-9 

I.I3I 

47-1 

28.13 

38.02 

63-4 

60 

1.050 

32-9 

1.058 

33-9 

37-64 

34-47 

49-9 

70 

0.972 

18.2 

o-975 

18.8 

46.28 

29-57 

3i-4 

80 

0.893 

6.4 

0.895 

6.6 

61  .15 

21.95 

13-3 

90 

0.837 

0.7 

0.838 

0.9 

71.18 

12.83 

2-3 

97-4 

0.8o6 

0.08 

0.808 

0.36 

77-39 

3.28 

o-5 

SOLUBILITY  OF  CANE  SUGAR  IN  AQUEOUS  ALCOHOL  SOLUTIONS  AT  14°. 

(Schrefeld  —  Z.  Ver.  Zuckerind.  44,  '971  '94.) 


Wt. 

Wt. 

Gms.  Sugar  per  100 

Wt. 

Wt. 

Gms.  Sugar  per  100 

>er  cent 

per  cent 

cc.  Alcohol-H2O 

per  cent 

per  cent 

cc.  Alcohof-H2O 

UcohoL 

Sugar. 

Mixture. 

Alcohol. 

Sugar. 

Mixture. 

0 

66.2 

195-8 

50 

38.55 

62.7 

5 

64.25 

179.7 

60 

26.70 

36-4 

10 

62  .20 

164.5 

70 

12.25 

13-9 

20 

58-55 

141  .2 

80 

4-05 

4.2 

30 

54-05 

II7.8 

90 

o-95 

0.9 

40 

47-75 

9I-3 

100 

o.oo 

o.o 

100  gins,  absolute  methyl  alcohol  dissolve  1.18  gms.  sugar  at  19°. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  784,  '92.) 

SOLUBILITY  OF  SUGARS  IN  PYRIDINE  AT  26°. 

(Holty  — J.  Physic.  Chera.  9,  764,  '04.) 


Sugar. 

T-         i                   Gms.  Sugar  per         Sp.  Gr.  of 
100  Gms.  Solution.       Solutions. 

Cane  Sugar 
Milk  Sugar 
Grape  Sugar 

C12H22On 
C12H22On.H20 
C6H120C.H20 

6-45 
2.18 
762 

0.9811 
i  .0521 

SUGAR  326 

SOLUBILITY  OF  CANE  SUGAR  IN  AQUEOUS  ACETONE  AT  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  41,  322,  '04.) 


Sp.Gr.of 
Solutions. 

cc.  Acetone 
per  loo  cc. 
Solvent. 

Cms.  Sugar 
per  loo  cc. 
Solution. 

Gms. 

per  100  cc.  Solution. 

H20. 

(CH3)2CO. 

Q2H22On 

•3306 
.2796 

0-0 
20-0 

89.8 
76.7 

43-3 

42.9 

o.o 

8.4 

89.8 
76.7 

.2491 
.2OO2 
.1613 

30.0 
4O.O 

45-o 

72.1 

59-3 
52-5 

39-5 
39-8 
39-o 

13-4 
20-9 
24.6 

72.1 

59-3 

52-5 

Above  45  cc.  acetone  per  100  cc.  solvent  the  solution  begins  to 
separate  into  two  layers.  The  lower  of  these  contains  51  gms.  sugar 
per  100  cc.  and  has  Sp.  Gr.  1.1522.  The  upper  layer  contains  so 
little  sugar  that  the  amount  could  not  be  determined  by  the  method 
employed.  100  cc.  evaporated  in  a  vacuum  desiccator  left  a  residue 
of  3.68  gms.  Above  the  concentration  of  80  cc.  acetone  per  100  cc. 
solvent  the  two  layers  unite.  In  pure  acetone  100  cc.  solution  give 
a  residue  of  0.18  gram  sugar. 

SOLUBILITY  OF  GRAPE  SUGAR  IN  WATER  AND  IN  AQ.  ALCOHOL. 

100  gms.  H2O  dissolve  81.68  gms.  C6H12O6  or  97.85  gms.  C6H12O6.H2O 
at  15°. 

100  gms.  aq.  alcohol  of  0.837  Sp.  Gr.  =  85  wt.  per  cent  dissolve 
1.95  gms.  C6H12O6  at  17.5°. 

100  gms.  aq.  alcohol  of  0.880  Sp.  Gr.  =  66  wt.  per  cent  dissolve 
B.io  gms.  C6H12O6  at  17.5°. 

100  gms.  aq.  alcohol  of  0.910  Sp.  Gr.  =  53  wt.  per  cent  dissolve 
16.01  gms.  C6H12O6  at  17.5°. 

100  gms.  aq.  alcohol  of  0.915  Sp.  Gr.  =  51  wt.  per  cent  dissolve 
32.50  gms.  C6H12O6  at  17.5°. 

SOLUBILITY  OF  MILK  SUGAR  IN  WATER  AND  IN  ABSOLUTE  METHYL 

ALCOHOL. 

100  gms.  H2O  dissolve  17.03  gms.  Ci2H22On.H2O  at  10°,  20.8  gms. 
at  25°  (U.  S.  P.),  40  gms.  at  100°,  and  100  gms.  at  b.  pt. 
100  gms.  abs.  methyl  alcohol  dissolve  0.084  gm-  at  19.5°. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  784,  '92.) 


SULPHANILIO    ACID  NH2.C6H4SO3H. 

SOLUBILITY  IN  WATER. 

(Dolinski  —  Ber.  38,  1836,  '05.) 

Gms.  Acid  per  100  Gms.  Gms.  Acid  per  100  Gms. 

Solution.          Water.  "  Solution.          Water.  " 

o    0.64    0.64       60    3-01    3-io 
10    0.83    0.84       70    3-65    3-78 

20      1.07      I. 08  80     4.32      4.51 

30    1.47    i-49       90    5-25    5-54 
40    1.94    1.97       100    6.26    6.67 

50   2.44   2.51 


327 


SULPHUR 


SULPHUR  S 

SOLUBILITY  IN: 

Tin  Tetra  Chloride. 

Amyl  Alcohol. 

(Gerardin 

—  Ann.  chim.  phys. 

[4]  5,  134.  '6s  •) 

(Gerardin.) 

t°. 

Cms.  S 
per  100  Gms. 
SnCl4. 

Solid 
Phase. 

t°. 

Gms.  S 
per  loo  Gms. 
C5HUOH. 

Solid 
Phase. 

99 

5-8 

Solid  S 

95 

I-5 

Solid  S 

101 

6.2 

« 

no 

2  .1-2  .2 

« 

no 

8.7-9.1 

« 

112 

2  .  6-2  .  7 

Liquid  S 

112 

9.4-9.9 

Liquid  S 

120 

3-o 

n 

121 

17.0 

i< 

131 

5-3 

« 

SOLUBILITY  OF  SULPHUR  IN  ETHYL  AND  METHYL  ALCOHOLS. 


15 

18.5 
b.  pt. 
18.5 


Alcohol. 


Abs.  Ethyl 


Abs.  Methyl 


Gms. 

per  too  Gms. 
Alcohol. 

0.051 

0-053 

0.42 

0.028 


Authority. 

(Pohl.) 

(de  Bruyn  —  Z.  physik.  Chem.  10,  781,  '92.) 
(Payen  —  Compt.  rend.  34,  356,  '52.) 
(de  Bruyn.) 


SOLUBILITY  OF  SULPHUR  IN  AQUEOUS  ACETONE  AT  25°. 

(Herz  and  Knoch  —  Z.  anorg.  Chem.  45,  263,  '05.) 


Wt.  per  cent 

Acetone 
in  Solvent. 

IOO 


90.62 

85-38 


Sulphur  per  100  cc. 
Solution. 

Millimols. 

Grams. 

65.0 

2.084 

45-o 

1-442 

33-o 

1.058 

25-3 

O.SlI 

Sp.  Gr. 
of 

Solution. 

0.7854 
0.79II 
0.8165 
0.8295 


SOLUBILITY  OF  SULPHUR  IN  BENZENE  AND  IN  ETHYLENE  Di 

BROMIDE. 

(Etard  —  Ann.  chim.  phys.  [7]  2,  571,  '94;  see  also  Cossa  —  Ber.  i,  139,  '68.) 

In  C2H4Br2. 


In 

C6H6. 

' 

Gms.  S 

Gms.  S 

t  °. 

per  loo  Gms. 

t°. 

per  loo  Gms. 

Solution. 

Solution. 

0 

I  .0 

70 

8.0 

10 

I  .3 

80 

10.5 

20 

1-7 

90 

13-8 

25 

2.1 

IOO 

17-5 

30 

2-4 

no 

23.0 

40 

3-2 

120 

29.0 

50 

4-3 

130 

36.0 

60 

6.0 

' 

Gms.  S 

Gms.  S 

t°. 

per  loo  Gms. 

t°. 

per  100  Gms. 

Solution. 

Solution. 

o 

1.2 

50 

6.4 

IO 

i-7 

60 

8.4 

20 

2-3 

70 

II-4 

25 

2.8 

80 

I6.5 

30 

3-3 

90 

24.0 

40 

4-4 

IOO 

36.5 

TOO  gms.  sat.   solution  of   S  in  benzoyl  chloride,  C7H7C1,  contain 
I  gram  S  at  o°  and  55.8  gms.  at  134°. 

(Bogousky  —  J.   Soc.  Phys.  Chim.  R.  37,  92,  '05.) 


SULPHUR  328 

SOLUBILITY  OF  SULPHUR  IN  CARBON  BISULPHIDE. 

5s;  at  10°,  Retgers 
ii,  274,  '95-96.) 


(Etard  —  Ann.  chim.  phys.  [7]  2,  571,  '94;  Cossa  —  Ber.  i,  138,  '65;  at  10°,  Retgers  —  Z.  anorg.  Chem 
3»  347.  '93;  below  —  77°,  Arctowski  — Ibid,  n, 


Cms.  S  per  joo  Cms.  Gms.  S  per  100  Gms.  Gms.  S  per  100  Gms. 

Solution.      CS2  Solution.          CS2.  "Solution.         CS2.    ' 

-no      3.0      3.1         -io        13.5         15.6          50      59.0       143.9 
— 100      3.5      3.6  o        18.0        22. o          60      66. o       194.1 

—  80   4.0   4.2     io    23.0*   29.9     70   72.0   257.1 

-  60    3-5    3-6        20     29.5     41.8      80    79.0    376.1 

-  40   6.0   6.4     25    33.5    50.4    90   86.0   614.1 

—  20  10.5  ii -7     30   38.0    61.3    100   92.0  1150.0 

40    50-0   100.0 

*  26.4  R. 

Sp.  Gr.  of  solution  saturated  at  15°  containing  26  gms.  S  per  100 
gms.  solution  =  1.372. 

SOLUBILITY  OF  SULPHUR  IN  HEXANE  (C6H14). 

(Etard.) 

A.O  Gms.  S  per 

100  Gms.  Solution. 

—  2O  O.O7 

O  O.l6 

20  0.25 

40  0.55 

SOLUBILITY  OF  SULPHUR  IN  SEVERAL  SOLVENTS. 

(Cossa  —  Ber.  i,  139,  '68;  Retgers;  Cap  and  Garot — J.  pharm.  chim.  [3]  26,  81  '54;  Kleven  —  Chem, 

Centralb.  434,  '72.) 

Gms.  S  per 
100  Gms.  Solvent. 

1.48 
10. 0  (R.) 
10.58 

O.O5-O.I  (C.andG.) 


SOLUBILITY  OF  SULPHUR  IN  COAL  TAR  OIL,  LINSEED  OIL  AND 
IN  OLIVE  OIL. 

(Pelouze  —  Compt.  rend.  68,  1179,  '69;  69,  56,  '69;  Pohl.) 
Grams  S  per  100  Grams  Coal  Tar  Oil  of: 


t°. 

Gms.  S  per 
100  Gms.  Solution. 

t°. 

Gms.  S  per 
100  Gms.  Solution. 

60 

I  .0 

130 

5-2 

80 

i-7 

140 

6.0 

100 

2.8 

160 

7.2 

1  20 

4-4 

180 

8.2 

Solvent. 

j.o          Gms.  S  per 
100  Gms.  Solvent 

Solvent. 

] 

C6H5NH2 
CHC13 

(C2H5)20 
C6H5OH 

130 
22 

23-5 

85-3 
I  .21 
0-97 

C6H5CH3 
CH2I2 
C10H4N2* 
C5H3(OH)3 

230 
10 
100 

ord.  t. 

*  Nicotine. 

A.O  Sp.Gr.:     0.87 
'  b.  pt.:  8o°-ioo°. 

0.88 

85°-I20°. 

0.882 

I20°-220° 

0.885             i  -oi 

.    I50°-200°.    2IO°-300°. 

1  .02 

220°-30O°. 

15 

2  .1 

2 

•3 

2 

•5 

2 

.6 

6. 

0 

7- 

o 

30 

3-0          4-0 

5 

•3 

5 

.8 

8. 

5 

8. 

5 

50 

5-2 

6 

.1 

8 

•3 

8 

•7 

io. 

0 

12  . 

o 

80 

ii.  8 

13 

•7 

15 

.2 

21 

.0 

37- 

0 

41. 

o 

100 

15.2 

18 

•7 

23 

•  O 

26 

•4 

S2- 

5 

54- 

o 

1  10 

23 

•  o 

26 

.2 

31 

•  o 

105. 

0 

115  . 

0 

120 

27 

.0 

32 

.0 

38.0 

00 

00 

130 

38 

•7 

43 

.8 

00 

00 

G.  S  per  100  Gms. 
Linseed 


Olive 
Oil  of 

vu-    0.885  Sp.Gr 
0-4  2.3 

0.6         4.3 

1.2  9-O 

2.2          l8.O 
3-0          25.0 

3-5      3o-o 

4.2     37.0 

5.0      43-0 

(160°)   io. o 

100  gms.  oil  of  turpentine  dissolve  1.35  gms.  S  at  i6°,and  16.2  gms. 

P  (Payen  —  Compt.  rend.  34,  356,  '52.) 


329 


SULPHUR    DIOXIDE 


SULPHUR    DIOXIDE   SO, 


SOLUBILITY  IN  WATER. 

(Schonfeld  —  Liebig's  Ann.  95,  5,  '55;   Sims  —  Ibid.  118,  340,  '61;  Roozcboom  —  Rcc.  trav.  chim.  3. 

46,   84.) 


Schonfeld. 

Vols.  SO2  (at  o°  and 
760  mm.)  per  i  Vol. 

Gms.  SO2  per 
loo  Gms.  HjjO 

Sims. 

SO2per  i  Gm.  H2O. 

Roozeboom. 

SO2  Dissolved 
per  i  pt.  HaO 

**' 

Sat.  SO2 

+  Aq. 

H20. 

at  total  pressure    t  °. 
760  mm. 

Gms. 

Vols." 

*   .        at  760  mm. 
pressure. 

O 

68.86 

79 

•79 

22 

•83 

8 

0.168 

58.7 

0 

O 

.236 

5 

59.82 

67 

.48 

19 

.31 

10 

0.154 

53-9 

2 

O 

.218 

10 

5I-38 

56 

•65 

16 

.21 

14 

0.130 

45-6 

4 

O 

.201 

15 

43-56 

47 

.28 

13 

•54 

20 

0.104 

36-4 

6 

0 

.184 

20 

36.21 

39 

37 

II 

.29 

26 

0.087 

30-5 

7 

O 

.176 

25 

30-77 

32 

79 

9 

.41 

30 

0-078 

27-3 

8 

O 

.168 

30 

25.82 

27 

16 

7 

,81 

36 

0.065 

22.8 

10 

o 

•154 

35 

21.23 

22 

49 

40 

0.058 

2O-4 

40 

17  .01 

18 

•77 

5 

,41 

46 

0.050 

17.4 

12 

o 

.142 

5° 

0.045 

I5.6 

Sp.  Gr.  of  sat.  solution  at  o°  =  1.061;  at  10°,  1.055;  a^  20°  =  1.024. 
i  gm.  H2O  dissolves  0.0909  gm.  SO2  =  34.73  cc.  (measured  at  25°) 
at  25°  and  748  mm.  pressure. 

(Walden  and  Centnerszwer  —  Z.  physik.  Chem.  42,  462,  'oi-'oa  . 


SOLUBILITY  OF  SULPHUR  DIOXIDE  IN  SULPHURIC  ACID  OF 


1.84  SP.  GR. 


Interpolated  from  original  results. 


(Dunn  —  Chem.  News,  45,  272,  '82.) 


Sp.  Gr. 

Coefficient 

Sp.  Gr. 

Coefficient 

of  Sat. 
Solution. 

of  Absorp- 
tion (760  mm.). 

t°. 

of  Sat. 
Solution. 

of  Absorp- 
tion (760  mm.) 

0 

53-o 

5° 

I.  8l86 

9-5 

10 

I  .8232 

35-o 

60 

1.8165 

7.0 

20 

I  .8225 

25.0 

70 

1.8140 

5-5 

25 

I.822I 

21  .O 

80 

1.8112 

4-5 

30 

I.82I6 

18.0 

90 

I.  8080 

4-0 

40 

I  .8205 

13.0 

SOLUBILITY  OF  SULPHUR  DIOXIDE  IN  AQUEOUS  SULPHURIC  ACID 

SOLUTIONS. 

(Dunn;  see  also  Kolb  —  Bull.  soc.  ind.  Mulhouse  —  222,  '72.) 


Sp.  Gr.  of 

Approximate 

Coefficient 

Sp.  Gr.  of 

Approximate 

Coefficient 

t°. 

H2S04 

Per  cent 

of 

t°. 

H2S04 

per  cent 

of 

Solution. 

H2S04. 

Absorption. 

Solution. 

H2S04. 

Absorption 

6.9 

•139 

2O 

48.67 

15 

2 

•173 

25 

31.82 

6.9 

.300 

40 

45-38 

16 

.8 

^S1 

21 

3I-56 

8.6 

.482 

58 

39  -91 

14 

.8 

•277 

36 

30.41 

9.8 

•703 

78 

29.03 

15 

.1 

•458 

56 

29.87 

5-5 

.067 

IO 

36.78 

15 

.6 

.609 

70 

25-I7 

6.0 

.102 

*5 

3.408 

15 

o 

•739 

81 

20.83 

For  Coefficient  of  Absorption,  see  Ethane  page  133. 


SULPHUR    DIOXIDE  330 

SOLUBILITY  OF  SULPHUR  DIOXIDE 

(Fox  —  Z.  physik.  Che 

Results  in  terms  of  the  Ostwald  Solubility  Expression.    See  page  105. 


SOLUBILITY  OF  SULPHUR  DIOXIDE  IN  AQUEOUS  SALT  SOLUTIONS. 

(Fox  —  Z.  physik.  Chem.  41,  461,  '02.) 


Salt  Solution. 

NH4C1 

0.5  Normal 
'25  =  34  •  58 

1.0  N. 

1-5 
38 

N. 
.06 

2.0  N. 

39-76 

2.5  N. 
41-37 

3-0  N. 
42.78 

NH4Br 

'25  =  36 

.25 

39 

-46 

42 

.78 

46.06 

49.17 

52 

•25 

NH4CNS 

'25  =  37 

•78 

42 

•74 

47 

.26 

52 

.26 

57-oi 

61 

.46 

NH4NO3 

'25  =  33 

.96 

35 

.07 

36-28 

37 

.27 

38.01 

39 

.14 

NH4NO3 

'35=23 

•35 

24 

•23 

24 

•78 

25 

•57 

26.66 

27 

•43 

(NH4)2S04 

'25  =  33 

•35 

33 

.82 

34 

•33 

34 

•95 

35-47 

35 

.96 

(NH4)2S04 

'35=22 

.91 

23 

.14 

23 

•49 

23 

•93 

24.23 

24 

.60 

CdCl2 

'25  =  3J 

.66 

30 

•55 

29 

.46 

28 

.16 

27.09 

26 

.06 

CdCL, 

'35=2I 

•73 

21 

•23 

20 

•55 

20 

.02 

19.23 

18 

.68 

CdBr2 

'25=  31 

.91 

31 

.01 

30 

29 

•27 

28.15 

27 

.46 

CdBr2 

'35=21 

.88 

21 

.46 

20 

.81 

20 

.60 

19.70 

19 

•17 

CdI2 

'25=33 

•27 

33 

.76 

34 

.16 

34 

•74 

34-98 

35 

•77 

CdI2 

'35=22 

•75 

23 

.06 

23 

•36 

23 

.71 

23-99 

24 

•30 

CdSO4 

'25=3! 

.11 

29 

.71 

28 

.24 

26 

•58 

25.14 

23 

•76 

CdS04 

'35=21 

•45 

20 

•43 

19 

.42 

18 

•31 

17.41 

16 

•25 

KC1 

'25=34 

.42 

36-05 

37 

•76 

39 

•32 

40.96 

42 

.27 

KC1 

'35=23 

•74 

25 

•15 

26 

•54 

27 

•94 

28-93 

30 

.02 

KBr 

'25=35 

•94 

39 

.11 

42 

.41 

44 

.96 

48.87 

52 

.26 

KBr 

'35=24-83 

27 

•49 

29 

.64 

31 

•93 

34.12 

36 

.14 

KCNS 

'25=37 

•57 

42 

•38 

47 

.02 

51 

.81 

55-87 

61 

.26 

KCNS 

'35=25 

-63 

28 

•79 

32 

•03 

35 

•05 

38-13 

42 

•94 

KI 

'25=38 

.66 

44 

•76 

50-58 

56 

•75 

62.63 

68 

•36 

KI 

'35=26 

•3° 

30 

•25 

34 

.64 

38 

.04 

41.87 

45 

•43 

KN03 

'25=33 

.80 

34 

•79 

35 

•77 

36 

.66 

37-57 

38 

•52 

KN03 

'35=23 

•27 

24 

•03 

24 

•79 

25 

•72. 

26.54 

27 

•33 

K2S04 

.20 

33 

.61 

NaBr 

'25=33 

•76 

34 

•54 

35 

.27 

36 

.26 

36-84 

37 

•74 

NaCl 

'25=32 

.46 

32 

•25 

.96 

.76 

3I-51 

31 

•36 

NaCNS 

'25=35 

•44 

38 

.24 

40 

•78 

43 

•37 

45-86 

48 

•34 

Na2SO4 

'25=31 

.96 

.14 

30 

•45 

29 

•51 

28.66 

28 

•44 

Na2SO4 

'35=21 

.88 

21 

•35 

20 

.81 

20 

.21 

19-75 

J9 

.27 

SOLUBILITY  OF  SULPHUR  DIOXIDE  IN  ALCOHOLS  AND  IN  OTHER 

SOLVENTS. 

(de  Bruyn  —  Rec.  trav.  chim.  u,  128,  '92;  Schulze  —  J.  pr.  Chem.  [2]  24,  168,  '81.) 

In  Ethyl  Alcohol        In  Methyl  Alcohol         In  Several  Solvents 
at  760  mm.  at  760  mm.  at  o°  and  725  mm.  (S.) 

jo        Gms. SC>2jper  100 Gms.       Gms.  SO2  per  too  Gms.  gi       *          SO2 per  i  Gm. Solvent. 

Solution.    C2HsOH.  Solution.    CH3OH.'  Grams.       Vols- ' 

o  53.5  115.0  71.1  246.0  Camphor      0.880  308 

7  45-0  81.0  59.9  149.4  CH3COOH  0.961  318 

12.3  39.9  66.4  52.2  109.2  HCOOH      0.821  351 

18.2  32.8  48.8  (17. 8°)  44.0  78.6  (CH3)2CO     2.07  589 

26.0  24.4  32.3  31.7  46.4  SO2C12          0.323  189 


331 


SULPHUR    DIOXIDE 


DISTRIBUTION  OF  SULPHUR  DIOXIDE  AT  20°  BETWEEN: 

(McCrae  and  Wilson  —  Z.  anorg.  Chem.  35,  n,  '03.) 


Water  and  Chloroform. 


Aq.  HC1  and  Chloroform. 


Cms.  SO2  per 
Liter  in: 

Gm.  Equiv.  ^SOj 
per  Liter  in: 

Cone. 

Gms.  SO2  per 
Liter  in: 

Gm.  Equiv.    $SO3 
per  Liter  in: 

Aq. 
Layer. 

CHC13 
Layer. 

Aq. 
Layer. 

CHC13 
Layer. 

of 
HC1. 

Aq. 

Layer. 

CHC13 
Layer. 

Aq. 
Layer. 

CHC1, 
Layer. 

I-738 

I 

.123 

O 

•0543 

O 

•0351 

0-05 

1.86 

I.46 

0-0581 

0.0456 

i-753 

j 

.122 

0 

•0547 

0 

•0350 

« 

3-07 

2.83 

0.0960 

0-0884 

2.346 

j 

•703 

0 

.0732 

0 

•0532 

n 

4.28 

4-07 

0.1336 

O.I27I 

2.628 

I 

.897 

0 

.0821 

0 

.0592 

(i 

5-34 

5-42 

0-1667 

0.1692 

3-058 

2 

•385 

0 

•0955 

0 

•0745 

0.10 

1.25 

1.41 

0.039 

O.O44 

3-735 

3 

.062 

0 

.1166 

0 

.0956 

(I 

2.78 

3.08 

0.0868 

0.0962 

4.226 

3 

.626 

0 

•1319 

0 

.1132 

n 

3-86 

4-08 

O.II99 

0.1275 

5.269 

4 

.798 

0 

.1645 

0 

.1498 

n 

5  .161 

5-72 

0.1612 

0.1784 

6.588 

6 

.183 

0 

.2057 

0 

.1930 

0.2 

1.268 

i-Si 

0.0396 

0.0471 

31.92 

33 

.84 

0 

.9968 

I 

.056 

« 

1,914 

2.27 

0.0597 

0-0710 

33-26 

37 

•25 

I 

.038 

I 

.163 

(t 

2.464 

3-04 

0.0769 

0.0949 

u 

3-967 

4.90 

0.1239 

0.1530 

0.4 

i  .202 

1.61 

0.038 

0.0504 

n 

1.894 

2  .26 

0.059 

0-0706 

TANNIC    ACID    C13H9O7COOH. 

100  gms.   H2O  dissolve  about  294  gms.  at  25°;  100  gms.  alcohol 
dissolve  about  439  gms.  at  25°.  (U.S. P.) 

TAETARIO    ACID    C2H2(OH)2(COOH)2. 

SOLUBILITY  IN  WATER. 

(Leidie  —  Compt.  rend.  95,  87,  '82.) 
t°.        Grams  Tartaric  Acid  per  100  Gms.  H2O.  t°.      Gms.  Tartaric  Acid  per  100  Grns.  H2O. 


' 

Dextro 

Racemic 

Racemic 

Dextro 

Racemic 

Racemic 

and  Laevo 

Ac. 

Ac. 

and  Laevo 

Ac. 

Ac. 

Acids. 

Anhydrous. 

Hydrated. 

Acids. 

Anhydrous. 

Hydrated 

O 

115.04 

8.16 

9-23 

50 

195.0 

5O.O 

59-54 

10 

125.72 

12.32 

14.00 

60 

217-55 

64.52 

78.33 

20 

139-44 

18.0 

2O.6o 

70 

243.66 

80.56 

99.88 

25 

147.44 

21.4 

24.61 

80 

273-33 

98.12 

124.56 

30 

156.2 

25  -2 

29.10 

90 

306.56 

117  .20 

I52-74 

40 

176.0 

37-o 

43-32 

100 

343-35 

I37-80 

184.91 

SOLUBILITY  OF  TARTARIC  ACID  IN  ALCOHOL  AND  IN  ETHER 

AT  15°. 

(Bourgoin  —  Ann.  chim.  phys.  [5]  13,  405,  '78.) 

Gms.  Tartaric  Acid  per  100  Gms. 
Solvem-  Sat.  Solution.  Solvent! 

Absolute  Alcohol  20.385  4i-i35 

90  %  Alcohol  29 . 1 46  25. 604 

Absolute  Ether  o .  389  o .  40 

TELLURIUM  Te. 

100  gms.  methylene  iodide  CH2I2  dissolve  o.i  gm.  Te  at  12°. 

(Retgers  —  Z.  anorg.  Chem.  3,  349.  '93) 


TELLURIC    ACID 


332 


TELLURIC    ACID  H2TeO4.2H2O. 

SOLUBILITY  IN  WATER. 

(Mylius  —  Ber.  34,  2208,  '01.) 


... 

Gms. 
H2TeO4 
per  100 
Gms.  Sol. 

Mols 
H2Te04  per         Solid 
100  Mols.        Phase. 
H20. 

to. 

Gms. 
H2TeO4 
per  loo 
Gms.  Sol. 

Mols. 
H2TeO4  per        Solid 
loo  Mols.         Phase. 
H20. 

o 

13.92 

1.51    H2Te04.6H20 

30 

33.36 

4.67   H2TeO4.2HjC 

5 

17.84 

2.03 

40 

36.38 

5-33 

10 

26.21 

3-31 

60 

43  -67 

7-04 

jt- 

32-79 

4.41 

80 

$1-53 

9-93 

10 

25.29 

3.15    H2Te04.2H20 

IOO 

60.84 

14.52 

18 

28.90 

3.82 

no 

67.0 

19.0             M 

TELLURIUM   DOUBLE  SALTS 

SOLUBILITY  OF  TELLURIUM  DOUBLE  BROMIDES  AND  CHLORIDES 
IN  AQUEOUS  HYDROCHLORIC  AND  HYDPOBROMIC  ACIDS 

AT    22°. 
(Wheeler  —  Z.  anorg.  Chem.  3,  432,  '93.) 


Tellurium  Double  .Salt. 


Formula. 


Solvent. 


Gms.  Double  Salt  per  100 
Gms.  Solvent 


Te  Caesium  Bromide      TeBr4.2CsBr    Aq.  HBr 
Te  Potassium.  Bromide      TeBr4.2KBr 
Te  Rubidium  Bromide 
Te  Caesium  Chloride 
Te  Rubidium  Chloride 


TeBr4.2RbBr 
TeCl4.2CsCl    Aq.  HC1* 
TeCl4.2RbCl 


of  i.4pSp.  Gr. 
0.02 

6-57 
0.25 
0.05 

of  i.o8Sp.Gr. 
0.13 
62.90 

3-88 
0.78 

o-34 

13.09 

So.  Gr.  of  Aq.  HC1  solutions  1.2  and  1.05  respectively. 


THALLIUM   ALUMS 


Alum. 


SOLUBILITY  IN  WATER  AT  25° 

(Locke  —  Am.  Ch.  J.  26.  174,  '01.) 

Salt  per  100  Grams  H2O. 
Formula. 


Tl  Aluminum  Alum 
Tl  Vanadium  Alum 
Tl  Chromium  Alum 
Tl  Iron  Alum 


Gms. 

Gms. 

Gm. 

Anhydrous. 

Hydrated. 

Mols. 

7-5 

11.78 

0.0177 

25-6 

43-31 

0-0573 

IO.48 

16.38 

0.0212 

36-IS 

64.6 

0.0799 

TlAl(SO4)2.i2H2O 
TlV(SO4)2.i2H9O 
TlCr(S04)2.i2H20 
TlFe(S04)2.i2H20 

THALLIUM   BROMATE   TlBrO3 

One  liter  saturated  aqueous  solution  contains  3.463  gms.  TlBrO3  at  19.96° 
(B.),  and  7.355  gms.  at  39-75°  (N.  and  A.). 

(Bottger  —  Z.  physik.  Chem.  46,  602,  '03;  Noyes  and  Abbott — Ibid.  16,  132,  'gs.) 

THALLIUM   BROMIDE  TIBr 

One  liter   saturated   aqueous   solution   contains  0.42   gm.   TIBr   at    18°, 
0.476  gm.  at  20°,  0.57  gm.  at  25°,  and  2.467  gms.  at  68.5°. 

(Kohlrausch — Z.  physik.  Chem.  50,  356,  '04;  Noyes — Ibid.  6,  248,  '90;  Bottger.) 

SOLUBILITY  or  TIBr  IN  AQ.  SOLUTIONS  OF  T1NO3  AT  68.5°.    (Noyes.) 

Gram  Molecules  per  Liter.  Grams  per  Liter. 


0.0163  T1NO, 
0.0294      ll 
0.0955      " 


0.00410  TIBr 
0.00289     " 
0.00148     " 


4.336  T1N03 
7.820      " 
25-400      " 


i .  164  TIBr 
0.821     " 
0.420     " 


333  THALLIUM    CHLORATE 

THALLIUM   CARBONATE  AND   THALLIUM    (Per)    CHLORATE. 
THALLIUM   CHLORATE  T1C1O3.  (See  P-  338-) 

SOLUBILITY  IN  WATER. 

(Muir  —  J.  Chem.  Soc.  29,  857,  '76.) 
t°  0°  20°  50°  80°  100° 

Gms.  T1C1O3  per  ioo  gms.  H2O     2.80    3.92     12.67     36-65     57 -31 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  THALLIUM  CHLORATE  AND 
POTASSIUM  CHLORATE  IN  WATER  AT  10°. 

(Roozeboom  —  Z.  physik.  Chem.  8,  532,  '91.) 

NOTE.  —  Solutions  of  the  two  salts  were  mixed  in  different  pro- 
portions and  allowed  to  crystallize,  such  amounts  being  taken  that 
not  more  than  one  or  two  grams  would  separate  from  one  liter. 


Grams  per  1000  cc. 
Solution. 

Mg.  Mols.  per  1000  cc. 
Solution. 

Sp.  Gr. 

of 

Mol.  per  cent 
KC1O3  in  Mixed 

TldlO3. 

KC103. 

T1C103. 

KC1O3. 

Solutions. 

Crystals. 

25.637 

89.14 

I  .0210 

O 

19.637 

6.884 

68.27 

56-I5 

I  .0222 

2  .0 

12  -OOI 

26.IOO 

41-73 

2  1  2  .  89 

I  .0278 

12  .6l 

9.036 

40-064 

31.42 

326.79 

I-0338 

25.01 

7.885 

7-935 

46.497 
46-535 

27.42 
27  .60 

379.26 

379-57 

I  .0360 

}     36.30-97-93 

6.706 

46.410 

23.32 

378.55 

1-0357 

99.28 

6.729 

47-109 

23-37 

384-25 

I  .0363 

99.60 

4.858 

47  -312 

16.89 

385-91 

I  -0345 

99.62 

2.769 

47-134 

9.63 

384.46 

I  .0330 

99.67 

49.925 

407.22 

1.0330 

IOO-OO 

SOLUBILITY  OF  MIXED  CRYSTALS  OF  THALLIUM  CHLORATE  AND 

POTASSIUM  CHLORATE  IN  WATER  AT  DIFFERENT 

TEMPERATURES. 

(Quoted  by  Rabe  —  Z.  anorg.  Chem.  31,  156,  '02.) 

TOO  gms.  HoO  dissolve  2.8  gms.  T1C1O3  4-  3.3  gms.  KC1O3  at  o°. 
100  gms.  H2O  dissolve  10.0  gms.  TICICX -f  i .  5  gms.  KC1O3  at  15°. 
100  gms.  H2O  dissolve  12.67  £ms-  T1C1O3  +  16.2  gms.  KC1O3  at  50°. 
100  gms.  H2O  dissolve  57.3  gms.  T1C1O,  +  48.2  gms.  KClO8at  100°. 


THALLIUM    CHLORIDE    T1C1. 


SOLUBILITY  IN  WATER. 


(Average  curve  from  results  of  Noyes  —  Z.  physik.  Chem.  9,  609,  '92;  Bottger  —  Ibid.  46,  602,  '03;  Kohl- 
rausch  —  Ibid.  50,  350,  '04;  Hebberling;  Crookes;  Lamy  —  The  results  of  Berkeley  —  Trans.  Roy. 
Soc.  (Lond.)  203  A,  208,  '04  are  also  given.) 

0 
10 
2O 

Gms.  T1C1 
Liter. 

per                 t0> 

Gms.  T1C1  per           t<> 
Liter. 

Gms.  T1C1  per 
Liter. 

2.1  (av.) 

2-5 
3-3 

I 
2 

3 

•7 
4 
•4 

(B.)  25 

30 
40 
5o 

3 

4 

5 
6 

.86 

.2 
.2 

•3 

4-0 

4.6 
6.0 
8.0 

60 
80 

100 

8.0 

12  -O 

18.0 

IO-2 

16.0 

24.1 

(99-3°) 

THALLIUM   CHLORIDE  334 

THALLIUM    CHLORIDE    T1C1. 


SOLUBILITY  IN  WATER  AND  IN  AQ.  SALT  SOLUTIONS  AT  25°. 

(Noyes;  Noyes  ar\d  Abbott;  Geffcken  —  Z.  physik.  Chem.  49,  296,  '040 
G.  Mols.  per  Liter.                          Grams  per  Later. 

/\Q.  oiiit  ooiution* 
Ammonixun  Nitrate  NEUNOs 

>i 

it 

Barium  Chloride  BaCl2 
Cadmium  Sulphate  CdSO4 

Hydrochloric  Acid  HC1 

'  Salt. 
0-0 

o-5 

I.O 
2.0 
0-0283 
0.1468 
0.030 
0.0787 

0.1574 
0.0283 
0-0560 

TICK 

o.  01612 

0.02587 
0.03I2I 
0.03966 
0.00857 
0-00323 
O.O2O6 
0.0254 
0.0309 
0.00836 
0-00565 

Salt. 

o.o 

40.02 

80.05 

160.10 
5-895 
30-59 
6-255 
16.41 

32.82 
1.032 
2.043 

T1C1. 

3.861  (G.) 

6.2O9 

7-473 
9-497 
2.052  (N.) 

0-773 
4-933  (N.) 
6.081 

7-399 

2.002   (N.) 

1-353 

14 

0.1468 

0.00316 

5-357 

o-757 

Lithium  Nitrate  LiNO3 

o-5 

O.O2542 

34-53 

6.o85(G.) 

" 

i  .0 

0-03035 

69.07 

7.266 

it 

2-O 

0-03785 

138.14 

9.063 

" 

3-o 

0.04438 

207.21 

10.630 

Potassium  Chlorate  KClOa 

o-5 

0.0237 

61.28 

5  674  (G.) 

Potassium  Nitrate  KNO3 

0-015 

O.OI7O 

i-5i7 

4-070  (N.) 

" 

0-030 

0.0179 

3-033 

4-286 

" 

0.0787 

O.OI92 

7-775 

4-597 

it 

o.i574 

O.O2I2 

15.920 

5.076 

M 

o-5 

0.0257 

50-55 

6.153(0.) 

M 

i  .0 

0.0308 

IOI.II 

7-375 

" 

2.0 

0.0390 

202.22 

9-340 

Sodium  Acetate  CHaCOONa 

0.015 

0.0168 

1.231 

4-023  (N.) 

" 

0.030 

O.OI72 

2.462 

4.118 

" 

0-0787 

0.0185 

6.46 

4-430 

" 

0-1574 

0.0196 

12.92 

4-693 

Sodium  Nitrate  NaNO» 

o-5 

0.02564 

42.50 

6.139  (G.) 

ii 

I.O 

0.03054 

85.01 

7-3I3 

" 

2.O 

0-03851 

170.02 

9.221 

ii 

3-o 

0.04544 

255-03 

10.88 

it 

4.0 

0.05128 

340.12 

12.28 

Sodium  Chlorate  NaClOj 

o-5 

O.O232O 

53-25 

5-555  (G.) 

I.O 

0.02687 

106.5 

6  -433 

2.0 

0.03060 

213.0 

7.326 

3-o 

0-03303 

3I9-5 

7.909 

41 

4-0 

0.03850 

426.0 

9.215 

Thallium  Bromate  TIBrOj  (at  39.75°) 

0.01567 

0.01959 

5  201 

4.690  (N.andA.) 

Thallium  Nitrate  T1NO« 

0.0283 

0.0083 

7.518 

1.987   (N.) 

0.0560 

O.OO57I 

14.89 

1.368 

" 

0.1468 

0.00332 

39-05 

0-795 

Thallium  Sulphate  T12SO4 

0.0283 

0.00886 

14.27 

/   SU 

2.  121  (N.) 

'    . 

0.0560 

0.00624 

28.23 

1-494 

Thallium  Sulphocyanide  T1SCN 

Sat. 

O.OII9 

Sat. 

2.849(N.) 

(at  39-75°) 

0.02149 

O.Ol8o7 

5-504 

4.326  (N.andA.) 

335 


THALLIUM   CHLORIDE 


SOLUBILITY  OF  THALLIUM  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OP 

SALTS  AT  25°. 

(Noyes  —  Z.  physik.  Chem.  9,  609,  '92.) 


Aq.  Salt               Gram.  Equiv.  per 

Liter. 

Grams,  per  Liter. 

Grams  per  Liter. 

Solution.        Salt. 

T1C1. 

Salt. 

T1C1.  ' 

Salt. 

T1C1. 

NH4C1 

o.o 

NH4C1  or  HC1 

0. 

Ol6l2 

0.00  NH4C1    3 

,861 

0 

.00 

HC1     3 

.861 

and 

also  0.025 

" 

O. 

00873 

1.338 

2. 

101 

0.886 

2, 

o 

HC1 

0.05 

11 

0. 

00589 

2.676 

"         I 

.421 

i 

•772 

I 

.402 

O.IO 

"               0.00384          .  .                           ... 

3 

•545 

"         0 

.920 

o.  20 

" 

0. 

00262 

10.  704 

0.649 

7 

.090 

44        O 

.608 

CuCl2 

0.025CuCl2or  CaCl20. 

00902 

3.36 

CuCl2  2 

.161 

3 

•77 

CaClj  2 

.161 

and 

also  0.05 

«« 

0. 

00619 

6.72 

I 

•483 

7 

•55 

I 

.483 

CaCl2 

O.IO 

" 

O. 

00419 

13-45 

I 

.003 

15 

.11 

44        I 

.003 

0.20 

" 

0. 

00287 

26.90 

"        O 

.688 

3° 

.22 

0 

.687 

MgCl2 

0  .  025MgCl2  or  MnClizO  . 

CKXJOl 

2.381 

MgCl2  2 

.158 

3 

.147 

MnCl2  2 

.158 

and 

also  0.05 

O.Oo6l8 

4.763 

"        1.480 

6 

•295 

I 

.480 

MnCl2 

O.  IO 

11 

0. 

00412 

9.526 

"        O 

.987 

12 

•59 

44        O 

.987 

0.20 

11 

0. 

00278 

19.052 

0 

.666 

25 

.18 

0 

.666 

KC1 

0.025 

KC1  or  NaCl 

0.00871 

1.86 

KC1    2 

.086 

I 

.46 

NaCl    2 

.086 

and 

also  0.05 

" 

O. 

00592 

3-73 

"        I. 

,418 

2 

•925 

I 

.418 

NaCl 

O.  IO 

" 

0. 

00397 

7.46 

"        0 

•951 

5 

•85 

44        0 

•951 

0.20 

0.00268 

14.92 

44      o 

.642 

ii 

.70 

44         O 

.642 

T1C1O 

3         0.025  TIClOaorTlNOsO  .  00889 

5.276 

T1C1O3  2 

.129 

4 

-74 

T1NO3  2 

.129 

and 

also  0.05 

•• 

0. 

00626 

9 

.48 

I 

.500 

T1NO3        o.io 

0 

,00423 

... 

18 

.96 

I 

.014 

ZnCl2 

0.025 

ZnCl2 

0.00899 

3-41 

ZnCl2  2 

•153 

0.05 

0.00627 

6.81 

44         I 

.502 

O.IO 

0.00412 

13-63 

"        0.987 

0.20 

" 

o. 

0028l 

27.26 

44         0 

•673 

CdCl2 

0.025 

CdCl2 

0.0104 

4-53 

CdCl2    2 

.491 

0.05 

" 

o. 

0078 

9.16 

"        I 

.868 

O.IO 

•' 

0. 

00578 

18.33 

I 

-385 

O.20 

"             0.00427 

36.66 

I 

.029 

One  liter  of  water  dissolves  2.7  gms.  thallo  thallic  chloride  jTlCl.TlCl, 
at  i5°-i7°,  and  35.0  grams  at  100°. 

(Crookes;  Lamy;  Hebberling.) 


THALLOUS  CHROMATE  Tl2CrO4. 

100  gms.  H2O  dissolve  0.03  gm.  Tl2CrO4  at  60°,  and  0.2  gm.  at  100°. 

(Browning  and  Hutchins  —  Z.  anorg.  Chem.  22,  380,  *oo.) 

One  liter  of  aq.  31  per  cent  KOH  solution  dissolves  18  grams  Tl2CrO4. 

(Lepierre  and  Lachand  —  Compt.  rend.  113,  196,  '91.) 

One    liter    of    H2O    dissolves    0.35    gram    Thallous    Tri    Chromate 
Tl2Cr3010  at  15°,  and  2.27  grams  at  100°.  (Crooke,.> 


THALLOUS   CYANIDE  336 

THALLOUS    CYANIDE     T1CN  and  Double  Cyanides. 
SOLUBILITY  IN  WATER. 

(Fronmuller  —  Ber.  n,  92,  '78.) 

Cyanide.  Formula.  Gms.  Salt  per  zoo  Cms.  H3O. 

Tl  Cyanide  T1CN  at  28.5°,  16.8 

Tl  Cobalti  Cyanide   Tl3Co(CN)6  at  o°,  3.6  ;  at  9.5°,  5.86  ;  at  19.5°,  10.04 

Tl  Zinc  Cyanide         2TlCN.Zn(CN)2       at  o°,  8.7  ;  at  14°,  15.2  ;  at  31°,  29.6 
Tl  Ferro  Cyanide       Tl4Fe(CN)6.2H2O     at  18°,  0.37     at  ioi5,  3.93. 

(Lamy.) 

THALLOUS    FLUORIDE  TIP. 

100  gms.  H2O  dissolve  80  gms.  TIP  at  15°. 

(Buchner  —  Sitzb.  K.  Akad.  Wiss.  (Wein)  52,  2,  644,  '65.) 

THALLIUM    IODATE    T1IO3. 

One  liter  aq.  solution  contains  0.578  gram  T1IO3  at  20°. 

(Bottger  — Z.  physik.  Chem.  46,  602,  '03.) 

THALLIUM    IODIDE    Til. 

SOLUBILITY  IN  WATER. 

(Average  results  from  Bottger;  Kohlrausch;  Werther;  Crookes;  Lamy;  Hebberling.) 

t  °.  o°.  20°.         40°.  60°.         80°.  100°. 

Gms.  Til  per  liter      0.02        0.06        0.15        0.35        0.70         1.20 

One  liter  of  z\  per  cent  aq.  ammonia  dissolves  0.761  gm.  T1C1. 
One  liter  of  6$  per  cent  aq.  ammonia  dissolves  0.758  gm.  T1C1. 
One  liter  of  90  per  cent  alcohol  dissolves  0.0038  gm.  T1C1. 
One  liter  of  50  per  cent  alcohol  dissolves  0.027     gm.  T1C1. 

(Long  — J.   Anal.  Ch.  2,  243,  '88.) 

THALLIUM    NITRATE    T1NO3. 

SOLUBILITY  IN  WATER. 

(Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203  A,  213,  '04;  see  also  Etard  —  Ann.  chim.  phys.  [7]  2, 
527,  '94;  Crookes;  Lamy.) 

Gms.  TlNO3-per  100  Gms.  Gms.  T1NO3  per  100  Gms. 


Solution. 

Water. 

i.  . 

Solution. 

Water. 

o 

3-76 

3-91 

60 

31-55 

46.2 

10 

5-86 

6.22 

70 

41  .01 

69-5 

20 

8.72 

9-55 

80 

52.6 

III  .O 

30 

12.51 

14-3 

90 

66.66 

2OO-O 

40 

J7-33 

20.9 

100 

80.54 

4I4-0 

5° 

23-33 

30-4 

105 

85-59 

594-0 

Solid  phase.     T1NO3  rhombic. 

100  gms.  H2O  dissolve  43.5  gms.  T1NO3  +  104.2  gms.  KNO3  at  58°. 

(Rabe  —  Z.  anorg.  Chem.  31,  156,  '02.) 

THALLIUM    OXALATE  T12C2O4. 

One    liter    of    saturated    aqueous    solution    contains  15.77    grams 
T12C2O4  at  20°,  and  18.69  £ms.  at  25°. 

(Bottger  — Z.  physik.  Chem.  46,  602,  '03;  Abegg  and  Spencer  — Z.  anorg.  Chem.  46,  406,  '05.) 


337 


THALLIUM   OXALATE 


SOLUBILITY  OF  THALLIUM  OXALATE  AT  25°  IN  AQ.  SOLUTIONS  OF: 


Thallium  Nitrate. 


(Abegg  and  Spencer.) 

Mol.  Concentration.  Grams  per  Liter. 

T1N03-      T12C204.~ 

o-oo     18.69 

10-95 
21  .26 


Potassium  Oxalate. 

(A.  and  S.) 


Mol.  Concentration. 


T1N03. 
O-O 

O.O4II4 
0.0799 
0-1597 


T12C204. 
0-03768 
0-0264 
0.0195 
0.01235 


K2C204.        T12C204. 
0-0498      0-0351 
0-0996      0-03565 
0-2467 
0.4886 


Grams  per  Liter. 

K2C204.     T12C204. 

8.28l    17.42 

16.57 


0.0390 
0-04506 


41  -02 
81.25 


17.69 
19.36 
22-37 
27.48 


13  .IO 
9-68 
42.51   6.128 

0.9785   0.05536  162.6 

THALLOUS    PHOSPHATE  (ortho)  T13PO4. 

One  liter  of   sat.  aqueous  solution  contains  4.97  gms.  T13PO4  at  15° 

(Crookes.) 

T10C6H2(N02)3. 


and  6.71  gms.  at  100°. 
THALLIUM    PICEATE 


SOLUBILITY  IN  WATER. 

(Rabe  —  Z.  physic.  Chem.  38,  179,  '01.) 


t°. 

Gms. 
T10C6H2(N02)3            Solid 
per  joo                    Phase. 

t  °. 

T10C6H2(N02)3        Solid 
per  TOO                  Phase. 

Gms.  H20. 

Gms. 

H02. 

0 

O  .  135         Monoclinic  Red 

45 

I 

.04 

Triclinic  Yellow 

18 

0.36 

47 

I 

.IO 

" 

30 

0-575 

50 

I 

.205 

" 

40 

0.825 

60 

I 

•73 

" 

45 

I  .01 

7o 

2 

•43 

" 

47 

1.14 

ioo   gms.    H2O    dissolve   0.132    gm. 
C6H4(NO2)3OK  at  o°. 

ioo  gms.   H2O  dissolve  0.352   gm. 
C6H4(N02)3OK  at  15°. 

ioo    gms.    H2O    dissolve    0.38    gm. 
C6H4(N02)3OK  at  20°. 


C6H2(NO2)3OT1  +  0.36   gram 
C6H2(NO2)3OT1  +  0.44     gram 


C6H2(NO2)3OT1  +  0.23 


gram 

(Rabe.) 


SOLUBILITY  OF  THALLIUM  PICRATE  IN  METHYL  ALCOHOL. 

(Rabe.) 


t°. 

Gms. 
T10C6H2(NO2)3               Solid 

Gms. 
t°.      T1OC6H2(NO2)3                    Solid 

per  ioo                      Phase. 
Gms.  CH3OH. 

per  100                            Phase. 
Gms.  CH3OH. 

0 

O-  39          ^e^  Form  (monoclinic). 

45 

i-i95 

Yellow  Form  (triclinic). 

18 

o-59 

48 

i.  265 

25 

o.  70 

50 

x'325 

" 

30 

0-795 

53 

1.41 

" 

35 

0.90 

57 

1-54 

" 

40 

1.02 

60 

1-65 

u 

45 

I.I7 

65 

1.84 

" 

47 

1.265 

THALLIUM   SULPHATE  338 

THALLIUM   SULPHATE   T12SO4. 

SOLUBILITY  IN  WATER. 

(Berkeley  —  Trans.  Roy.  Soc.  (Lond.)  203  A  211,  '04;  see  also  Crookes;  Lamy.) 


Gms.  T12SO4 

per 

IOO 

Gms.  T12SO4 

per  ioo 

;e.                            Gms.                                       t°. 

Gms 

Solution. 

Water. 

Solution. 

Water. 

0 

2.63 

2. 

70 

60 

9.89 

10.92 

10 

3-57 

3- 

70 

70 

11.31 

12-74 

2O 

4.64 

4- 

87 

80 

12.77 

I4.6l 

30 

5.80 

6. 

16 

90 

14.19 

16  -53 

50 

8.44 

9- 

21 

99-7 

15-57 

18.45 

ioo  gms.  H2O  dissolve  4.74  gms.  T12SO4  +  10.3  gms.  K2SO4  at  15°. 
100  gms.  H2O  dissolve  11.5  gms.  T12SO4  +  16.4  gms.  K2SO4  at  62°. 
ioo  gms.  H2O  dissolve  18.52  gms.  T12SO4  +  26.2  gms.  K2SO4  at  100°. 

(Rabe  —  Z.  anorg.  Ch.  31,  156,  '02.) 

THALLIUM    SULPHIDE  T12S. 

One  liter  of  sat.  aqueous  solution  contains  0.215  gm.  T12S  at  20°. 

(Bottger  —  Z.  physic.  Chem.  46,  602,  '03  7 

THALLIUM  DOUBLE  SULPHATES 

SOLUBILITY  IN  WATER  AT  25°. 

(Locke  —  Am.  Ch.  J.  27,  459,  '01.) 

Salt  per  TOO  cc.  H2O. 

Double  Sulphate.  Formula. — : — - — " — rr-», 

Gms .  Anhydrous .     Gram  Mols . 

Tl  Copper  Sulphate  Tl2Cu(SO4)2.6H2O  8.1          0.0122 

Tl  Nickel  Sulphate  Tl2Ni(SO4)2.6H2O  4.61         0.007 

Tl  Zinc  Sulphate  Tl2Zn(SO4)2.6H2O  8.6          0.0129 

THALLIUM  SULPHOCYANIDE  T1SCN. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  SALT  SOLUTIONS. 

(Bottger;  Noyes;  Noyes  and  Abbott.) 

One  liter  sat.  aq.  solution  contains  3.154  gms.  T1SCN  at  20°,  3.905  gms. 
at  25°,  and  7.269  gms.  at  39.75°. 

Aq.  Salt  Solution.  t°.  ^  M°1S'  ""  ^  GBUM  *" Uta' 


Salt.  T1SCN.  Salt.  T1SCN. 

Thallium  Chloride  T1C1  25  sat.  O.OIO7  sat-  2  •  805  (N.) 

Thallium  Bromate  TIBrO.  39-75       0.014960.0221  4  .  966  5  .  793  (N.  and  A.) 

Thallium  Nitrate  T1NO»  25  O.O227      0.00852  6.04  2.233   (N'> 

25    0.0822  0.00406  21.88  1.064 

Potassium  Sulphocyanide,  KSCN    25  O.O227      0.0083          2  .  208    2  .  176  (N.) 

THALLIUM    CARBONATE    T12CO3. 

SOLUBILITY  IN  WATER. 

(Crookes;  Lamy.) 

t°  15.5°        18°        62°          100°      100.8° 

Gms.  T12CO3  per  ioo  gms.  H2O    4.2(0.)    5.23     12.85     27.2(0022.4 

THALLIUM   (Per)   CHLORATE  T1C1O4. 

ioo  grams  H3O  dissolve  10  gms.  T1C1O4  at  15°,  and  166.6  gms.  at  100°. 

(Roscoe  —  J.  Chem.  Soc.  19,  504,  '66.) 


339  THALLIUM    SULPHITE 

THALLIUM    SULPHITE  T12SO3. 

100  gms.  H2O  dissolve  3.34  gms.  T12SO3  at  15.5°. 

(Seubert  and  Elkeu  —  Z.  anorg.  Chem.  a    434,  '92.) 


THALLIUM    VANADATES. 

SOLUBILITY  IN  WATER. 

(Carnelly  —  J.  Chem.  Soc.  [2]  n,  323,  '73;  Laebig's  Ann.  116,  155,  '60.) 

Vanadate.  Formula.  Gms.  Vanadate  per  TOO  Gms.  H2O. 

At  15  .  At  100°. 

Tl.  meta  Vanadate  T1VO3  0.087(11°)  0.21 

"    ortho  Vanadate  T13VO3  i  .o  1.74 

"    pyro  Vanadate  T14V2O7  0.20(14°)  0.26 

"    Vanadate  T112V8O26  0.107  0.29 


THEOBROMINE  C5H2(CH3)2N4O2. 

100  gms.  carbon  tetra  chloride  dissolve  0.0212  gm.  at  b.  pt. 
100  gms.  ether  dissolve  0.032  gm.  at  b.  pt. 

(Gockel  — Chem.  Centralb.  ii,  401,  '97.) 

80   cc.    H2O   containing    14.8   gms.    tri   sodium   phosphate   dissolve 
3.5  gms.  theobromine  at  15°. 

(Brisse-Moret  —  J.  pharm.  chim.  [6]  7,  176,  '98.) 

THORIUM    SELENATE  Th(SeO4)4.9H2O. 

100  gms.  H2O  dissolve  0.498  gm.  Th(SeO4)4  at  o°  and  1.972  gms. 
at  100°. 

(Cleve  —  Bull.  Soc.  chim.  [2]  43,  166,  '85.) 

THORIUM    SULPHATE  Th(SO4)2. 

SOLUBILITY  IN  WATER. 

(Roozeboom  —  Z.  physic.  Chem.  5,  201,  '90;  Demarcay  —  Compt.  rend.  96,  1860,  '83.) 

Gms.  Th(S04)2  per  Solid  to       Gms.  Th(SO4)2  per  Solid 

'      100  Gms.  H20.     '  Phase.  100  Gms.  H2O.  Phase. 

O      0-74(R)     0.88(D)  Th(S04)2.9H20         O  I-5O(R)  Tb(SO4)2.6H2O 

10      0.98  1-02  "  15  1-63 

20       1.38  1.25  "  30  2-45 

30     1.995         I-&5  45  3-85 

40       2  . 998  2  . 83  60  6  . 64 

50     5. 22(51°)  4-86  ••  17  9-4i(D) 

55     6.76          6-5±  "  40    4-Q4(R)4-5(35°D) 

O      1-0  ThCSO^-SHa         50      2.54  1.94(55°) 

15       1.38  60      1.63 

25       1.85  "  70      1-09  I-32(750) 

44    3-7i  "  95       •••         o-7i 


TIN    CHLORIDE  340 

TIN    CHLORIDE  (Stannous)    SnCl2. 

100  gms.  H2O  dissolve  83.9  gms.  SnCl2  at  o°  and  269.8  gms.  at  15°, 
Sp.  Gr.  of  Solutions  1.532  and  1.827  respectively. 

(Engel  —  Ann.  chira.  phys.  [6]  17,  347,  '89;  Michel  and  Krafft  —  Ibid.  [3]  41,  478,'  51.) 

SOLUBILITY  OF  STANNOUS  CHLORIDE  IN  AQUEOUS  SOLUTIONS  OF 
HYDROCHLORID  ACID  AT  o°. 

(Engel.) 


Milligram  Mols. 
Solution 

per  10  cc. 

Sp.  Gr. 

of 

Grams  per  ioo  cc. 
Solution. 

HC1. 

}SnCl2. 

Solution. 

HC1. 

SnCl2. 

0 

74-o 

1-532 

o.o 

70.26 

6.6 

66.7 

1.489 

2.405 

63-33 

13-54 

63-7S 

1.472 

4-935 

60.52 

24.8 

68.4 

1.524 

9.04 

64-95 

34-9 

8l.2 

I  .625 

12.72 

77.11 

40-0 

94.2 

1.724 

14.58 

89-45 

44.0 

II7.6 

1.883 

16.04 

111.7 

49-4 

147.6 

2.II4 

18.01 

138.6 

66.0 

156.4 

2  .190 

24.05 

148.5 

78.0 

J57-o 

2.199 

28.43 

149-0 

100  gms.  acetone  dissolve  55.6  gms.  SnCl2  at  18°. 

(Naumann  —  Ber.  37,  4332,  '04.) 

ioo  gms.  ether  dissolve  11.4  gms.  SnCl2.2H2O  at  o°-35.5°. 

100  gms.  ethyl  acetate  dissolve  31.2  gms.  SnCl2.2H2O  at  —  2°,  35.53 

gmS.   at     +22°  and   73.44  gmS.   at  82°.  (von  Laszcynski  —  Ber.  27,  2285,  '94.) 

TIN    HYDROXIDE    Sn(OH)2. 

SOLUBILITY  IN  AQUEOUS  SODIUM  HYDROXIDE  SOLUTIONS.     MOIST 
TIN  HYDROXIDE  USED,  ORDINARY  TEMPERATURE. 

(Rubenbauer  —  Z.  anorg.  Chem.  30,  335,  '02.) 


Gms.  per  20  cc. 
Solution.                  D 

ilution  of  the 
NaOH. 

1.86 
1.25 
0.72 

Gms.  per  20  cc. 
Solution.                     j 

Mol. 
dilution  of  the 
NaOH. 

0.48 
0.23 

Na. 

o  .  2480 

0.3680 
0.6394 

Sn. 
0.1904 
0-2614 
0.4304 

Na. 
0.8326 
0.9661 
2.1234 

Sn. 
0.5560 
0.7849 
1.8934 

TIN    IODIDE    (Stannous)  SnI2. 

SOLUBILITY  IN  WATER  AND  IN  AQUEOUS  HYDRIODIC  ACID. 

(Young  —  J.  Am.  Chem.  Soc.  19,  851,  '97.) 
t°.  Gms.  SnI2  per  ioo  Gms.  Aqueous  HI  Solutions  of: 


o%  =  H20. 

5-83%. 

9-6o%  . 

15-2%. 

20.44%. 

24-8%. 

30.4%. 

36.82%. 

20 

0.98 

0-20 

0.23 

0.60 

1.81 

4.  20 

10.86 

25-31 

30 

1.16 

0.23 

0.23 

0.64 

1.81 

4.06 

10.28 

23.46 

40 

i  .40 

o-33 

0.28 

0.71 

1.90 

4.12 

10.  06 

23  -*5 

50 

i  .69 

0.46 

0.38 

0.82 

2.12 

4-34 

Jo-35 

23.76 

60 

2.07 

0.66 

o-55 

i  .11 

2.51 

4-78 

11.03 

24.64 

70 

2.48 

0.91 

0.80 

i-37 

2  .92 

5-43 

11.97 

25-72 

80 

2-95 

1.23 

1-13 

1.83 

3-70 

6.38 

I3-3Q 

27.23 

90 

3-46 

1-65 

1.52 

2.40 

4-58 

7.82 

I5-52 

29.84 

IOO 

4-03 

2  .23 

2.04 

3-63 

5-82 

9.60 

34-05 

341  TIN    IODIDE 

TIN   IODIDE    (Stannic). SnI4. 

SOLUBILITY  IN  CARBON  BISULPHIDE. 

(Sneider  —  Pogg.  Ann.  127.  624,  '66;  Arctowski  —  Z.  anorg.  Chem.  ix,  274,  '95.) 
t°-  -ii40-S    '    -94°  -89°  -84°  -58°          ord.  temp. 

Gms.  SnL  per  , 

ioo  gms  Solution      9"*1      10.65      9.68      10.22      16.27      59^(S.) 

ioo  gms.  methylene  iodide,  CH2I2,  dissolve  22.9  gms.  SnI4  at  10°. 
Sp.  Gr.  of  Solution  3.481. 

(Retgers  —  Z.  anorg.  Chem.  3,  343,  '93.) 


TIN    SULPHATE    (Stannous)  SnSO4. 

ioo  gms.  H2O  dissolve  18.8  gms.  SnSO4  at  19°  and  18.1  gms.  at  100°. 

(Marignac.) 

TOLUENE   C.H5CH,. 

SOLUBILITY  IN  SULPHUR. 
Figures  read  f-om  curve,  synthetic  method  used,  see  Note,  page  9. 

(Alexejew  —  Ann.  Physik.  Ch.  28,  305,  '86.) 

Gms.  C6H5CH3  per  ioo  Gms.  Gms.  CeHsCHa .per  ioo  Gms 

*°'  S  Toluene  *  °'  S  Toluene 

Layer.  Layer.  Layer.  Layer. 

ioo  3  73  150      12.5  59 

no  4  71  160      16  53 

'120  5  68  170      22  47 

130  7  66  175      25  43 

140  9.5  63  178  crit.  temp.  34 


TOLUIC  ACIDS  (Monomethyl  Benzoic  Acids)  CH3.CCH,.COOH. 

SOLUBILITY  IN  WATER  AT  25°. 

(Paul  —  Z.    physik.  Chem.  14,  in,  '94.) 


per  Liter  Solution. 
Acid'  Grams.  Millimols*. 

Meta  Toluic  Acid  0.9801  7.207 

Ortho  Toluic  Acid  i  .  1816  8  .683 

Para  Toluic  Acid  0.3454  2  .540 


TOLUIDINE  Cf)H4CH3.NH2. 

SOLUBILITY  IN  WATER. 

(Vaubel  —  J.  pr.  Chem.  [2]  52,  72,  '95;  Lowenherz  —  Z.  physik.  Chem.  25,  410,  '98.) 

Gms.  Gms. 

t  o  CeKUCHs-NHa  Solid  t  0  C^CHaNI^  Solid 

per  1000  Phase.  per  1000  Phase. 

Gms.  H2O.  Gms.  H2O. 

2O  16.26  Liquid  ortho  T.  2O-8  7 '39  ParaT. 

2O  O.I5  Ortho  T.  26.7  9-5° 

20  6.54  P^T.  31.7  11.42 


TOLUIDINE  342 

SOLUBILITY  OF  PARA  TOLUIDINE  IN  ETHYL  ALCOHOL. 

(Interpolated  from  original  results  of  Speyers  —  Am.  J.  Sci.  [4]  14,  295,  '02.) 


Wt. 

Mols.  per 

Gms.  per 

t  ° 

of  i  cc. 

ioo  Mols. 

ioo  Gms. 

Solution. 

C2H6OH. 

C2H5OH. 

O 

0-8885 

20.72 

48.1 

5 

0-8982 

26.0 

6o-O 

10 

0.9080 

32.0 

74.0 

15 

0.9180 

38.6 

9O.O 

... 

Wt. 
of  i  cc. 
Solution. 

Mols.  per 
ioo  Mols. 
C2H5OH. 

Gms.  per 
ioo  Gms. 
C2H6OH. 

2O 
25 

30 

0.9265 
0.9360 
0.9460 

47-0 

56.0 

66.0 

IIO.O 
132.0 
156.0 

Distribution   of   para  Toluidine  between   water   and   carbon    tetra 

Chloride.  (Vaubel  —  J.  pr.  Chem.  [2]  67,  478,  '03.) 


Gms.  p  Toluidin 
Used. 

I  .0 
1.0 


Volumes  of  Solvents. 

200  cc.  H2O-f  ioo  cc.  CC14 

200  CC.  H2O  +  200  CC.  CC14 


Gms.  CaH4(CH3)NH2  p  in: 
H20  Layer.  CCU  Layer." 
0.1406  0.8594 

0.0666  0.9334 


URANYL    CHLORIDE   UO2C12.3H2O. 

ioo  gms.  H2O  dissolve  320  gms.  UO2C12  at  18°. 

(Mylius  and  Dietz  —  Ber.  34,  2774,  '01.) 


URANYL  DOUBLE  CHLORIDES. 

SOLUBILITY  OF  URANYL  AMMONIUM  CHLORIDE,  U.  TETRA  METHYL 
AMMONIUM  CHLORIDE,  U.  TETRA  ETHYL  AMMONIUM  CHLORIDE, 
U.  CAESIUM  CHLORIDE,  U.  RUBIDIUM  CHLORIDE,  AND  U.  POTAS- 
SIUM CHLORIDE  IN  WATER. 

(Rimbach  —  Ber.  37,  463,  '04.) 


Formula  of 
Double  Salt. 


Gms.  per  ioo  Gms.  Sat.  Solution.        Atomic  Relation  in  Sol. 


Solid 
Phase. 


ri  i  Mol.  double  salt 
3-590  4-o.4Mol.NH4O 


29.8 

19.85  "    - 

-  io.44O2   =  41.24* 

iUO2:  4.020 

Double  salt 

80.7 

20.23 

-  io.52O2   —    4.91  * 

iU02:  3-98O 

" 

27.1 

15.02 

'    - 

-    7.81  C12   =37.I5t 

iU02:  3-97C1 

M 

80.7 

15-12 

-    7-7802   =  37-23  1 

iUO2:3-94O 

" 

29-75 

24.8 

22.11 
27.18 

-  22.5  Cs   =  56.04$ 
-i  6.6  Rb  -f-i3.8Cl§ 

iUO2:  2.o7Cs 
iUO2:  i.o6Rb:  3.900 

H 

80.3 

30.66 

-  19.1  Rb  - 

hi  5-80  || 

iUO2:i.98Rb:3-95Cl 

" 

0.8 

38.57 

-  13.590    - 

-    3-86K 

iUO2:2.69Cl:o.69K 

^ 

14.9 

33-71 

-13.510    - 

-    T..K 

iUO2:  3-o6O  :i.o6K 

The  double  salt 

17-5 

37-36 

-  14.500    - 

-    5-27K 

iU02:  2.96O  :  o.o6K 

J    is  decomposed 

25x5 

35-oi 

_ 

-  15.260    - 

-    ...  K 

iU02:3.33Cl:i.33K 

>  by    water     at 

35-27 

-15.920   - 

u    7-39K 

iU02:3.44Cl  :i.44K 

temperatures 

5° 

34-iS 

-16.560   - 

-    ...  K 

iU02:3.7iCl  :i.7iK 

below  60°. 

60 

34-19 

-  17.250   - 

-    9.1  4K 

iU02:  3-850  :i.85K 

J 

71  5 

33-55 

-    9-28K 

iU02:  3.96O  :i.96K 

Double  salt 

78-5 

35-26  "     - 

-  18^240    - 

-    9-95K 

i  UO2  13.950  :i.95K 

UOaCl2.2N(CH3)4O,  t  UO2a2.N(C2H6)4O,  i  UO2Cl2.2CsCl, 

§  =  57-9  gms.  UO2Cl2.2RbO2,  ||  =  65.8  gms.  UOxCb 


343  URANYL    SODIUM 

CHROMATE 
URANYL    SODIUM    OHROMATE  2(UO2)CrO4.Na2CrO4.ioH2O. 

100  gms.  sat.  aqueous  solution  contains  52.52  gms.  (2UO2).CrO4. 
Na2CrO4  at  20°.  (Rimbach.) 

URANYL  POTASSIUM  BUTYRATE    UO2(C4H7O2)2.KC4H7O2- 

The  double  salt  is  decomposed  by  water  at  ordinary  temperatures 
and  the  solution  gets  richer  in  uranyl  butyrate.  The  solubility  at 
29.4°  in  water  containing  KC4H7O2  is  2.10  gms.  UO2(C4H7p2)  +  0.38 
gms.  KC4H7O2  per  100  gms.  solution.  The  atomic  relation  being  i :  0.64. 

(Rimbach.) 

URANYL    NITRATE    UO2(NO3)2.6H2O. 

SOLUBILITY  IN  WATER,  ETC. 

(Bucholz;  de  Coninck  —  Compt.  rend.  130,  1304,  'oo.) 

ioo  gms.  cold  water  dissolve  200  gms.  UO2(NO3)2.6H2O. 
100  gms.  abs.  alcohol  dissolve  333  gms.  UO2(NO3)2.6H2O. 
ioo  gms.  85%  alcohol  dissolve  3.3  gms.  UO2(NO3)2.6H2O  at  12°  (de  C.) 
ioo  gms.  ether  dissolve  25  gms.  UO2(NO3)2.6H2O. 
ioo  gms.  abs.  acetone  dissolve  1.5  gms.  UO2(NO3)2.6H2O  at  12°  (de  C.) 
For   densities    of    Uranium    nitrate    solutions    in  water   and   other 
solvents  see  de  Coninck  —  Compt.  rend.  131,  1219,  'oo.) 


URANYL    DOUBLE    NITRATES. 

SOLUBILITY  OF  URANYL  AMMONIUM  NITRATE,  U.  CAESIUM 

NITRATE,  U.  POTASSIUM  NITRATE,  AND  U.  RUBIDIUM 

NITRATE  IN  WATER. 

(Rimbach.) 

Gms.  per  ioo  Gms.  Sat.  Solution. 
UO2.  Total  Salt. 

29.71  +  2.92NH4—     .  .  .       lUO2 
36.46+  3.54   "     ==68.95  " 

44.37+  2.90   "      -    ... 
44.95+  2.98   "     =78.95 
31.39+  6.59  Cs  =55.4 
31.98+  1.72  K    : 
33.40+  2.72  " 
37.07+4.01  "  *=  64.82 
42.18+  5.16  "    =    ... 
41.65+  6.03  "    =    ... 
43.71  +  6.38  "      =    .  .  . 
35.41+  4-65Rbf — 59-60 
34.66+11.01  "    =69.49 

*  +  23.5NO-3.  t  +  I9.74NG-3. 


Formula  of  4,  o 

Salt. 

U02(N03)2.NH4N03  0.5 
24.9 

59  -° 

"  80.7 

UO2(NO3)2.CsNO,     16.0 

U02(N03)2.KN03       0.5 

13.0 

25.0 


80.6 

UO2.(NO3)2.RbNO3  25.0 
80.0 


Atomic  Relation 

in  Solution. 

i.47NH4: 

3-47N03 

1.46  "     : 

3-46  " 

0.98  "     : 

2.98  " 

i.  oo  "     : 

3.00  " 

0.44  Cs 

2.37N03: 

0.37  K 

2-57  "     : 

0-57  " 

1.60  "    : 

0.76  " 

2.84  "     : 

0.84  " 

3.00  "    : 

1.  00    " 

3.01  "     : 

I.OI    " 

1.40  "    : 

o-45Rb 

3.00  "     : 

I.OI    " 

URANYL    AMMONIUM   PROPIONATE    2UO2(C3H6O2)2.NH4C3H8O2. 
2H2O  and  Uranyl  Potassium  Propionate  2UO2(C3H5O2)2.KC3H5O2. 

(Rimbach.) 

ioo  gms.  aq.  solution  contain  16.48  gms.  2UO2(C3H5O2)2.NH4C3H6O, 
at  29.8°. 

ioo  gms.  aq.  solution  contain  2.362  gms.  UO2(C3H5O2)2  +  0.82  gm. 
KC3H6O2  at  29.4°,  atomic  relation,  1:1.29. 


UBANYL  SULPHATE        344 

UBANYL  SULPHATE  (UO)2SO4.3H2O. 

SOLUBILITY  IN  WATER,  ETC. 

(Bucholz;  de  Coninck  —  Bull.  Acad.  Roy.  Belgique,  350,  *oi.) 

ioo  gms.  H2O  dissolve  16.6  gms.  UO2(SO4).3H2O  at  13.2°,  17.4  gms. 
at  15.5°,  and  22.2  gms.  at  b.  pt. 

ioo  gms.  abs.  alcohol  dissolve  4.0  gms.  UO2(SO4).3H2O  at  18.2° 
and  5.0  gms.  at  b.  pt. 

ioo  gms.  85%  alcohol  dissolve  2.6  gms.  UO2(SO4).3H2O  at  16°. 

ioo  gms.  16.2%  alcohol  dissolve  12.3  gms.  UO2(SO4).3H2O  at  10°. 

URANYL    POTASSIUM    SULPHATE  UO2SO4.K2SO4.2H2O 

ioo  gms.  sat.  aq.  solution  contain  10.41  gms.  UO2SO4.K2SO4  at  25° 
and  23.13  gms.  at  70.5°.  (Rimbach.) 

SOLUBILITY  OF  UO2SO4.2K2SO4.2H2O  +  UO2SO4.K2SO4.2H2O  IN  WATER. 

Gms.  per  ioo  Gms.  Solution.  Atomic  Relation  in  Sol.          Mol.  %  in  Solid  Phase. 


I    . 

UO2. 

* 

s 

34. 

UOj 

.      ] 

t. 

S04. 

Mono  Salt. 

Di  Salt.  ' 

14 

0.85 

4 

.19 

5 

•7i 

i 

35 

75  : 

18.88 

29 

71 

50 

6.70 

8 

15 

12 

•37 

i 

5 

20  : 

8.40 

76 

24 

80 

14.29 

8 

54 

J5 

•53 

i 

4 

I3  : 

3.06 

12 

88 

UREA    CO(NH2)2. 

SOLUBILITY  IN  WATER  AND  IN  ALCOHOLS. 

(Campetti  —  Abstract,  Z.  physic.  Chem.  41,  109,  '02;  Speyers  —  Am.  J.  Sci.  [4]  14,  259,  '02.) 

NOTE.  —  Speyer's  original  results  are  in  terms  of  Mols.  CO(NH2)2 
per  ioo  Mols.  H2O  at  irregular  temperatures. 

In  Water.  In  Methyl  Alcohol.  In  Ethyl  Alcohol. 


t  o           Wt.  Of   I   CC. 

Solution. 

Gms.  CO(NH2)2  per         Wt.  of  i  cc. 
looGms.  H2O.                   Solution. 

Gms. 
CO(NH2)2 
per  ioo  Gms. 

Gms. 
Wt.  of  ice.    CO(NH2)2 
Solution,    per  ioo  Gms 

CH3OH. 

.C2H5OH. 

0            1.  121 

55 

•9 

0.861 

13.8 

0.8213 

2-5 

IO 

•134 

66 

.0 

85.0 

(C) 

0.863 

16.0 

O.8l4 

3-5 

20       j 

.146 

79 

.0 

108.2 

(C) 

0.869 

20.  o 

0.809 

5-o 

30 

.156 

93 

•  O 

0.876 

24.0 

0.8o6 

6-5 

40 

.165 

106 

.0 

.  .  . 

0.890 

30.0 

0.804 

8-5 

50 

•173 

120 

.0 

.  .  . 

0.908 

37-o 

0.803 

10.5 

60 

.!80 

I32 

.0 

.  .  . 

0.928 

47-o 

13  .0 

70 

.187 

145 

.0 

*7-5 

ioo  gms.  abs.  methyl  alcohol  dissolve  21.8  gms.  CO(NH2)2  at  19.5°. 
ioo  gms.  abs.  ethyl  alcohol  dissolve  5.06  gms.  CO(NH2)2  at  19.5°. 

(de  Bruyn  —  Z.  physic.  Chem.  10,  784,  '92.) 

ioo  gms.  glycerine  dissolve  50  gms.  urea  at  15.5°. 

Phenyl  Thio  UREA  (Phenyl  thio  carbamide)   CS.NH2.NHC6H5. 
SOLUBILITY  IN  WATER. 

(Rothmund  —  Z.  physic.  Ch.  33,  406,  'oo;  Biltz  —  Ibid.  43,  42,  '03;  Holeman  and  Antusch  —  Rec.  trav. 
chim.  13,  200,  '94;  Bogdan  —  Ann.  Scien.  L'Univ.  Jassy  2,  43,  '02. '03.) 

One  liter  aq.  solution  contains  2.12  gms.  CS(NH2).NHC6H5  at  20° 
(B.),  (R.)  and  2.4  gms.  at  25°.  (H.  and  A.).  Bogdan  gives  2.547  gms 
at  25°. 


345 


Phenyl  Thio  UREA 


SOLUBILITY  OP  PHENYL  THIO  UREA  IN  AQUEOUS  SALT 
SOLUTIONS  AT  20°. 

(Biltz;  Rothmund.) 

Mfflimols  and  also  Cms.  CS(NH2)NHCftH5  Dissolved  per  Liter  of  Aqueous 
Salt  Solution  of  Concentration: 


Salt 

0.125  Normal 

0.25  Normal 

o.^  Normal 

ixs  Normal 

Solution. 

Millimols.     Gms. 

Millimols. 

Gms.    Millimols. 

Gms. 

Millimols. 

Gms. 

JA1C13 

12.95 

1.97 

12 

.82 

I 

.96 

12.03 

1.83 

10 

.69 

1.61 

NH4NO3 

14.17 

2.15 

14 

•4 

2 

.21 

J4-53 

2  .22 

14 

.91 

2.27 

i(NH4)2S04 

I3-51 

2.05 

12 

.84 

I 

.96 

11.78 

1-79 

9 

.98 

1.52 

iBaC!2 

13.12 

1.99 

12 

.92 

I 

•97 

12  .22 

1.86 

IO 

•44 

J-59 

JBa(N03)2 

13.98 

2.13 

13 

.98 

2 

•J3 

13.90 

2.12 

CsN03 

14-53 

2.21 

14 

.90 

2 

.27 

!5-23 

2-33 

. 

.  .  . 

LiN03 

13.96 

2.13 

J3 

.96 

2 

•13 

J3-93 

2  .12 

J3 

•73 

2.10 

iMgS04 

13.40 

2  .04 

12 

.78 

I 

•95 

n-54 

J-75 

9 

•43 

i-43 

KC2H3O2 

13.40 

2  -04 

12 

•95 

I 

•97 

12  .14 

1.85 

10 

•74 

1.62 

KBr 

13-50 

2.05 

J3 

•35 

2 

.04 

12.  80 

i-95 

ii 

.76 

1.79 

KC103 

13.86 

2.  II 

13 

.60 

2 

.06 

13.12 

1.99 

KC1 

13.40 

2  .04 

12 

•73 

I 

•94 

12  .19 

1-85 

10 

•54 

i.  60 

Kl 

14.12 

2.15 

14 

.48 

2 

.21 

I4-31 

2.18 

14 

.60 

2.23 

KN03 

13.89 

2  .12 

13 

•85 

2 

.11 

I3-52 

2.05 

12 

.82 

i  .96 

KNO2 

14.52 

2  .21 

14 

•65 

2 

•23 

13.80 

2  .11 

12 

•51 

1.92 

iK2S04 

13-25 

2.03 

12 

•49 

I 

.91 

ii  .11 

I  .69 

8 

•73 

i-33 

RbN03 

14.22 

2  .l6 

14 

•44 

2 

.19 

14-39 

2.18 

14 

.22 

2.17 

iNa2CO3 

13.29 

2  .04 

12 

•52 

I 

.9I 

ii  .05 

1.68 

8 

•58 

1.32 

NaClO3 

13-75 

2.09 

J3 

•65 

2 

.08 

13.07 

1.98 

12 

.21 

1.86 

NaC104 

14-15 

2.15 

14 

•05 

2 

.14 

I3-58 

2.06 

12 

•56 

1.92 

NaCl 

13.28 

2.02 

12 

•83 

I 

•95 

ii  .90 

1.81 

10 

.02 

1.52 

Nal 

13.98 

2.13 

14 

.07 

2 

.14 

14.29 

2.18 

J3 

.96 

2.13 

NaNO3 

13-94 

2  .12 

13 

•77 

2 

.10 

J3-32 

2  .04 

12 

•57 

1.92 

NaN02 

14-34 

2.18 

J3 

.82 

2 

.11 

13.06 

1.98 

II 

•52 

i-75 

iNa2S04 

13  -19 

2  -OO 

12 

•35 

I 

.s? 

10.85 

1.63 

8 

•30 

1.27 

SOLUBILITY  OF  PHENYL  THIO  UREA  AT  25°  IN  AQUEOUS 
SOLUTIONS  OF. 


Potassium  Nitrate. 

(Bogdan.) 

Sodium  Nitrate. 

(Bogdan.) 

Gms.  Mols. 
KN03  per 

Gms.  per 
1000  Gms.  H2O. 

Gms.  Mols. 
NaN03  per 

Gms.  per 
looo  Gms.  H2O. 

1000  Gms. 
HzO. 

KNO3. 

CS(NH2) 
.NHCeHs. 

1000  Gms. 
H20. 

NaNOa. 

CS(NH2) 
.NHQjHs. 

1.045 

105-7 

2-38 

I  .024 

87.14 

2.26 

o-5I23 

5I-84 

2.48 

0.5065 

43-10 

2.46 

O.2O26 

20.50 

2-54 

0.2031 

17.28 

2    51 

o  .  1007 

10.19 

2-56 

0.0986 

8-39 

2-53 

0-0503 

5-09 

2-55 

0-0540 

4-59 

2.54 

0-0333 

3-36 

2-55 

0-0335 

2.84 

2  54 

Phenyl  Thio  UREA 


346 


SOLUBILITY  OF  PHENYL  THIO  UREA  IN  MIXTURES  OF  ETHYL 
ALCOHOL  AND  WATER  AT  25°. 

(Holleman  and  Antusch  —  Rec.  trav.  chim.  13,  290,  '94.) 


Vol. 

Gms. 
CS(NH2) 

Sp.  Gr. 

per  cent 

NHQjHs 

of 

Alcohol. 

per  100  Gms. 

Solutions. 

Solvent. 

roo 

3-59 

95 

4-44 

O.82OO 

90 

4.69 

0.8389 

85 

4.99 

0.8544 

80 

4-70 

0.8679 

75 

4-45 

0.8810 

70 

3-92 

0.8915 

Vol. 

Cms. 
CS(NH2) 

Sp.Gr. 

per  cent 
Alcohol. 

NHC«H5 
per  zoo  Gms. 

of 
Solutions. 

Solvent. 

65 

3-40 

O.QOlS 

60 

2.80 

0.9128 

50 

1.87 

0.9317 

40 

I-I3 

o  .  9486 

25 

0.56 

0.9679 

IS 

0.38 

0.9788 

O 

0.24 

0.9979 

SOLUBILITY  OF  PHENYL  THIO  UREA  IN  AQUEOUS  SOLUTIONS  OF 
PROPYL  AND  OF  ETHYL  ALCOHOL  AT  25°. 

(Bagdan.) 


In  Propyl  Alcohol. 


In  Ethyl  Alcohol. 


G.  Mols. 

Gms.  per  1000  Gms.  H2O 

G.  Mols. 

Gms.  per  1000  Gms.H2O 

CaHyOH  per 
looo  Gms. 

C3H7OH. 

CS(NH2) 

NHPcHe 

C2HsOH  per 
1000  Gms. 

CzHsOH. 

CS(NH2) 

H20. 

11  v^6  £1-5  • 

H2O. 

UfttlS- 

I-03S 

62  .IO 

3.587 

I  .1010 

49.60 

3.193 

0.5448 

32.688 

3.124 

0-5355 

24.12 

2.931 

o  •  1059 

6-354 

2.643 

o  .  1094 

4-932 

2.629 

0-05526 

3-3J6 

2-599 

0.05018 

2.26 

2.589 

0-04854 

2  .912 

2.586 

0.03271 

1-473 

2-577 

In  Propyl  Alcohol  at  o°. 
i. ooo  60.06  i. 21 

o.ioo  6.01  1-047 


SOLUBILITY  OF  PHENYL  THIO  UREA  IN  AQUEOUS 
ACETONE,  MANNITE,  CANE  SUGAR,  DEXTROSE, 

(Bagdan.) 


Aqueous 
Non  Electro- 
lyte. 

(CR,)2CO 


C6H8(OH), 


SOLUTIONS  OF 
AND  UREA. 


; 

Gms 

.  per  1000  Gms. 
H?0 

Aqueous 
Non  Electro- 

to 

Gms.  per  1000  Gms. 
H20. 

* 

Non 

Elec- 

CS( 

NH2) 

lyte. 

• 

Non 

Elec- 

CS(NH2) 

trolyte. 

NH 

-CeHs. 

trolyte.        NHCeHg. 

25 

7 

-478 

2 

.667 

C.H,20, 

25 

180-40 

3 

.042 

2 

.513 

2 

•579 

ft 

tt 

90 

.46 

2 

•83 

tt 

I 

.908 

2 

•573 

tl 

it 

29 

.29 

•2 

.69 

it 

182 

•  II 

3 

.04 

tt 

(i 

18 

•  OI 

•  2 

•654 

it 

91 

•05 

2 

.78 

It 

" 

9 

•554 

2 

.603 

25 

338 

.6 

3 

•457 

CO(NH2)2 

it 

63 

.08 

3 

.306 

tt 

170 

•4 

3 

•015 

It 

tt 

29 

93 

2 

.892 

" 

34 

•36 

2 

•634 

It 

it 

6.132 

2 

.618 

ft 

18 

.28 

2 

•596 

tt 

it 

4 

942 

L  a 

•605 

11 

10 

.09 

2 

•572 

tl 

ti 

2 

.009 

2 

•572 

O 

342 

.18 

j 

420 

tl 

O 

60 

.11 

•t 

.310 

tt 

34 

.22 

I 

•044 

11 

n 

6 

.01 

i 

.048 

347 


URETHANE 


URETHANE     CO(NH2)OC2H5.     SOLUBILITY  IN  SEVERAL  SOLVENTS. 

(Speyers— Am.  J.  Sci.  [4]  14,  294,  '02.)    See  also  Ethyl  Carbamate,  p.  138. 

Interpolated  and   calculated   from   the   original   results  which   are 
given  in  terms  of  molecules  Urethane  per  100  Mols.  solvent. 


Solubility  in  Water. 


Solubility  in  Methyl  Alcohol. 


f. 

Wt     r                       M°IS- 

i  cc?           CO(NH2) 
Cr,!,,"           OC2Hg  per 
100  Mols. 

Gms 
CO(NH2) 
OC2H8per 
100  Gms. 

/  — 
Wt.  of 

I   CC. 

Solu- 

Mols. 
CO(NH2) 
OC2H6per 
100  Mols. 

Gms. 
CO(NH2) 

100  Gms 

tlon>                H20. 

H2O. 

tion. 

CH3OH. 

CH3OH. 

0 

1.023              3.61 

I7.8 

0.956 

3I.I8 

86.76 

10 

1.033          6-0 

29.7 

0.977 

41.0 

II4.I 

15 

1.042            15.0 

74-2 

0.989 

47-5 

132  .1 

20 

1.  060            3I-O 

153-3 

i  .000 

54-5 

IS1-? 

25 

1.073        5°-° 

247-3 

1.013 

62.5 

J73-9 

30 

1.078        65.0 

321.4 

1.024 

72.0 

200.3 

40 

1.065        77.0 

380.7 

1.045 

89.0 

247.7 

Solubility  in  Ethyl 

Alcohol. 

Solubility 

in  Propyl  Alcohol. 

to. 

Wt     nf                   Mols. 

,   '               CO(NH2) 
Solu             OC2H5per 
££             zoo  Mols. 

Gms. 
CO(NH2) 
OC2H5  per 
100  Gms, 

Wt.  of 

I   CC. 

Solu- 

Mols. 
CO(NH2) 
OC2HS  per 
100  Mols. 

Gms. 
CO(NH2) 
OC2H6  per 
100  Gms. 

C2H6OH. 

C2H5OH. 

tion. 

C3H7OH= 

O 

0.8914         23.91 

46.26 

0.880 

19.48 

28.9 

IO 

0-930           36.0 

69.6 

0.906 

31.0 

46.0 

15 

0.950           43.0 

89.2 

0.923 

40.O 

59-3 

20 

0.968            5O.O 

96.7 

0.942 

51.0 

75-7 

25 

0.985            59.0 

II4.I 

0.963 

6o-0 

89.0 

30 

i  .001         70.0 

135-4 

0.983 

68.0 

100.9 

40 

1.035         88-o 

170.2 

1.025 

85.0 

126.1 

Solubility  in  Chloroform. 

Solubility  in  Toluene. 

t° 

Wt.  of          C0(NH2) 

Gms. 
CO(NH2) 
OC2H5  per 

Wt.  of 

I  CC. 
O_l,, 

Mols. 
CO(NH2) 
OC2H6  per 

Gms. 
CO(NH2) 
OCsH  per 

S.?lu~            xoo2Mols. 

100  Gms. 

oOlU- 

100  Mols. 

100  Gms. 

tion.              CHC13. 

CHC13. 

tion. 

C6H6CH3. 

o 

1.404            27.56 

20.  6 

0.887 

1.77 

I.7I 

10 

1.340            41 

30.6 

0.874 

4.84 

15 

"I.3IO            46 

34-4 

0-875 

IO-O 

9.68 

20 

1.280        53 

39-6 

0-883 

16.0 

I5.48 

25 

1.240        60 

44.8 

0.902 

25.0 

24.18 

30 

1.203        67 

50.0 

0.927 

44-o 

42.58 

40 

1.125        80 

59-7 

o-995 

85.0 

82.24 

URIC 

ACID  C6H4N408. 

SOLUBILITY  IN  WATER. 

(Blarez  and  Deniges  —  Compt.  rend.  104,  1847,  '87;  at  15°  Magnier 
483,  '75-) 

—  Bull.  Soc. 

chim.  [2]  23, 

Gms.  C5H4N403. 

Gms. 

CsHiNtOi 

Gms.  C6H4N4O 

t  °. 

per  too  Gms. 

t°.             per 

TOO  Gms. 

t°. 

per  100  Gms. 

H20. 

H20. 

H20. 

O 

O.OO2 

30            o 

.0088 

70 

0-0305 

IO 

0.0037 

40            o 

.OI22 

80 

0.0390 

15 

0.0053 

50            o 

.0170 

00 

o  .  0498 

20 

0.006 

60            o 

.0230 

100 

0-0625 

VALERIANIO    AGID  348 

VALERIANIC    ACID  n  CH3(CH2)3COOH    (n    Propyl    acetic    acid — 
Pentane  acid)  when  shaken  with  water  at  16°  two  layers  are  formed. 

100  gms.  of  the  aqueous  layer  contains  3.4  gms.  CH3(CH2)3COOH. 
100  gms.  of  the  acid  layer  contains  90.4  gms.  CH3(CH2)3COOH. 

(Lieben  and  Rossi  —  Liebig's  Ann.  159,  60,  '71.) 

YTTRIUM  IODATE  Y(IO3)3.3H2O. 

100  gms.  H2O  dissolve  0.53  gm.  yttrium  iodate. 

(Berlin.) 

YTTRIUM    SULPHATE  Y2(SO4)3. 

100   gms.   H2O   dissolve    15.2   gms.   Y2(SO4)3  at   ord.   temperature, 
9.3  gms.     Y2(SO4)3.8H2O  at  ord.  temp,  and  4.8  gms.  Y2(SO4)3.8HO2 

at  IOO   .  (Cleve  —  Bull.  soc.  chim.  [2]  21,  344,  '74.) 

YTTERBIUM    SULPHATE  Yb2(SO4)3.8H2O. 
SOLUBILITY  IN  WATER. 

(Cleve  —  Z.  anorg.  Chem.  32,  143,  '02.) 


Gms.  Yb2(SO4)a 

Gms.  Yb2(SO4)3 

Gms.  Yb2(S04)3 

per  TOO  gms. 

t  °. 

per  loo  Gms. 

t°. 

per  loo  Gms. 

H20. 

H20. 

H20. 

44-2 

55 

"-S 

80 

6.92 

34-6 

60 

10.4 

90 

5-83 

19.1 

70 

7.22 

IOO 

4.67 

35 

ZINC    ACETATE  Zn(CH3COO)2.2H2O. 

loo  gms.  H2O  dissolve  40  gms.  at  25°  and  66.6  gms.  at  b.  pt. 
loo  gms.  alcohol  dissolve  2.8  gms.  at  25°  and  166.0  gms.  at  b.pt. 

(U.  S.  P.) 

ZINC    BENZOATE  Zn(C7H6O2)2. 

SOLUBILITY  IN  WATER. 

(Paietta  —  Gazz.  chim.  ital.  36,  II,  67,  '06.) 

t°.  15-9°     17°     27.8°     31.3°    37.5°  49.8°     59° 

Gms.  Zn(C7H5O2)2  per 
ico  gms.  aq.  solution        2.55    2.49     2.41       2.05      1.87     1.62     1.45 

ZINC    BROMIDE  ZnBr2. 

SOLUBILITY  IN  WATER. 

(Dietz  —  Wiss.  Abh.  p.  t.  Reizhanstalt  3,  431,  'oo;  see  also  Etard  —  Ann.  chim.  phys.  [7]  2,  536,  '94.) 


te. 

Gms.  ZnBr2 
per  loo  Gms. 
Solution. 

Mols.  ZnBr2 
per  loo 
Mols.H2O. 

Solid 
Phase. 

to. 

Gms.  ZnBr2 
per  100  Gms. 
Solution. 

Mols.  ZnBr2 
per  loo 
Mols.H20. 

Solid 
Phase. 

—  15 

77-13 

27.0 

ZnBr2.3H2O 

25 

82.46 

37-6 

ZnBr2.2H2O 

—  10 

78.45 

29.1 

" 

30 

84.08 

42-3 

" 

-  5 

80.64 

33-3 

" 

37 

86.20 

50.0 

" 

—  8 

79.06 

30-2 

ZnBr2.aH2O 

35 

85  -45 

46.9 

ZnBr2 

0 

79-55 

31  .1 

11 

40 

85-53 

47-4 

" 

+  13 

80.76 

33-5 

" 

60 

86.08 

49-5 

" 

18 

81.46 

" 

80 

86.57 

" 

IOO 

87-05 

53-8 

* 

349 


ZING  CARBONATE 


ZINC  CARBONATE  ZnCO,. 

One  liter  H2O  dissolves  o.oi  gm.  at  15°. 

One  liter  aq.    5.85   per  cent   NaCl   solution   dissolves   0.0586   gm. 
at  14°. 

One  liter  aq.   7.45  per  cent  NaCl   solutions  dissolves  0.0477  g111- 

«^k  J4   •  (Cantoni  and  Passamanik  —  Ann.  chim.  anal.  appl.  10,  258,  '05.) 

ZINC    CHLORATE  ZnClO3. 

SOLUBILITY  IN  WATER. 

(Meusser  —  Ber.  35,  1417,  '02;  at  18°;  Mylius  and  Funk  —  Ber.  30,  1718,  '97.) 


-18 
o 
8 

15 
18 


Cms. 
Zn(C103)2 
per  loogms. 

Solution. 

55-62 
59-19 
6O.2O 
67.32 
66.52 


Mols. 
Zn(C103)2 

per  100 
Mols.H20. 

9.70 

II.OS 
II-72 
15.96 
15-39 


Solid 
Phase. 


Zn(C103)2.6H20 


Zn(C103)2.4H20 


Cms. 
to.        Zn(C103)2 
per  jooGms. 
Solution. 

Mols. 
Zn(C103)2           Solid 
per  100              Phase. 
Mols.  H20. 

3O       76.66 
4O      69.06 

1  6.  20      Zn(C108)24H2O 
17.29 

55     75-44 
Ice  curve 

24.00 

-13     30.27 
-  9     26.54 

3.36                Ice 
2.8o 

Sp.  Gr.  of  solution  saturated  at  18°  =  1.916. 

ZINC    CHLORIDE  ZnCl2. 

SOLUBILITY  IN  WATER. 

(Mylius  and  Dietz  —  Z.  anorg.  Chem.  44,  217,  '05;  see  also  Dietz  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  429, 
'oo;  Etard  —  Ann.  chim.  phys.  [7]  2,  536,  *94-) 


AO        Gms.ZnCbper  looGms.             Solid 

A0    Gms.ZnCl2per  looGms.         Solid 

Water. 

Solution. 

Phase. 

"    Water. 

Solution. 

Phase. 

•  5 

14 

12 

•3 

Ice 

9 

360 

78.3 

.2*H20  +  .H2O 

10 

25 

2O 

.0 

" 

6 

385 

79-4 

ZnCl2.2iH20 

•40 

83 

45-3 

6 

298 

74-9 

ZnCla.iiHjjO 

-62 

IO4 

51 

.0 

ICe  +  ZnCl24H20 

10 

330 

76.8 

" 

•50 

113 

53 

.0 

ZnCl2.4H2O 

20 

368 

78.6 

" 

•40 

127 

55 

•9 

" 

26 

423 

80.9 

•i*H20+ZnC!2.H2O 

•30 

160 

61 

•5 

.4H20  +  .3H20 

26.3 

433 

81.2 

.1  *H20  -f-  ZnCl2 

-10 

189 

65 

•4 

ZnCl2.3H2O 

o 

342 

77-4 

ZnCl2.H2O 

o 

208 

67 

•5 

" 

IO 

364 

78.4 

" 

•   5 

230 

69 

•7 

" 

20 

396 

79.8 

" 

6-5 

252 

•4  71 

.6 

«• 

28 

436 

81.3 

ZnCl2.H20  +  ZnClj 

5 

282 

73 

.8 

» 

31 

477 

82.7 

ZnCIa.H20 

0 

309 

75 

•5 

.3H20  +  .i*H20 

25 

432 

81.2 

ZnCla 

o 

235 

70 

.1 

ZnCb.2iH.jO 

40 

452 

81.9 

" 

6.5 

252 

71 

.6 

.2iH2O  +  .3H2O 

60 

488 

83.0 

" 

10 

272 

73 

.1 

ZnCl2.2*H20 

80 

543 

84-4 

ii 

12.5 

303 

75 

.2 

'< 

IOO 

615 

86.0 

" 

"•5 

335 

77 

•  O 

.2*H20  +  .i*H20 

262 

00 

100-0 

" 

ZINC    CYANIDE    Zn(CN)2. 

loo  cc.  concentrated  Zn(C2H3O2)2  +  Aq.  dissolve  0.4  gm.  Zn(CN),. 
loo  cc.  concentrated  ZnSO4  +  Aq.  dissolves  0.2  gm.  (joannis.) 


ZINC    CHLORIDE 


350 


SOLUBILITY  OF  ZINC  CHLORIDE,  AMMONIUM  CHLORIDE  MIXTURES 


Isotherm  for  o°. 


IN  WATER. 

(Meerburg  —  Z.  anorg.  Chem.  37,  212, 

Isotherm  for  20°. 


Isotherm  for  30°. 


Gms.  per  ioo  Gms. 
Solution.              jSplid 

Gms.  per  ioo  Gms. 
Solution.                  Solid 

T>U  « 

Gms.  per  ioo 

Solution. 

Gm< 

Solid 
-,      Phase. 

ZnCl2. 

NH4Ci: 

'   ZnCl2. 

NH4C1. 

ZnCl2. 

NH.C1. 

O 

22 

.  8          NH4C1 

O 

.0 

26 

.  9          NHiCl 

O 

.0 

29 

•5 

NH4C1 

3-5 

23 

•  O 

5 

.1 

27 

.1               " 

9 

.2 

29 

•4 

" 

23 

•5 

9 

•5 

27 

•4 

16 

•  O 

29.7 

IO.2 

23 

•9 

12 

•7 

27 

•5 

20 

.2 

30 

.1 

" 

15  .1 

24 

•7 

15 

•7 

27 

•7 

24 

•7 

30 

•4 

«• 

18.0 

25 

•3 

18 

.0 

27 

•9 

26 

•3 

30 

.8 

NH4C1  +  a 

22  .4 

26 

.0 

23 

•5 

29 

.0 

27 

.2 

30 

.2 

a 

24.2 

26 

.  i 

26 

.0 

29 

•  5       NH4Cl  +  a 

30 

.1 

29 

.6 

" 

25-7 

26 

•3       NH4Cl+a 

29 

•5 

28 

.1                a 

36 

.8 

28 

.2 

" 

27-5 

26 

•  4               o 

32 

•3 

27 

•7 

42 

•4 

27 

•3 

" 

30-7 

25 

•7 

35 

.8 

27 

.0 

43 

.8 

27 

•3 

a  +  b 

33-9 

25 

•3 

38 

•7 

26 

•9 

45 

•  o 

24 

•4 

b 

38.8 

24 

•4 

40 

.2 

26 

.6 

51 

.2 

17 

.6 

» 

42  .6 

24 

•6           a  +  b 

41 

•9 

26 

•3 

61 

•9 

10 

•4 

" 

44-3 

21 

•3           b 

43 

.2 

26 

•O            a  +  fr 

66 

•9 

9 

.2 

ZnCl2  +  6 

49-2 

15 

46 

•9 

21 

.0                b 

75 

.6 

6 

.1 

ZnCl2 

52.6 

II 

•9 

53 

.2 

14 

•5 

70 

•3 

7 

.6 

« 

55-4 

10 

.0          «• 

58 

•4 

II 

.1 

78-5 

3 

.2 

«« 

59-3 

7 

•5 

62 

•7 

8.7 

76 

•9 

3 

•5 

it 

62.1 

6 

.8 

66 

.6 

7 

.9 

79 

.8 

i 

.6 

14 

81 

.6 

0 

.0 

M 

a  =  ZnCl2.3NHCl3,.    b  =  ZnCl2.2NH4Cl. 

ioo  gms.  abs.  acetone  dissolve  43.5  gms.  ZnCl2  at  18°. 

(Naumann  —  Ber.  37,  4332,  '04.) 

ioo  gms.  glycerine  dissolve  50  gms.  ZnCl2  at  15.5°. 

ZINC    FLUORIDE    ZnF2.4H2O. 

One  liter  of  water  dissolves  16  gms.  at  18°. 

(Dietz.) 

ZINC    HYDROXIDE    Zn(OH)2. 

One  liter  of  water  dissolves  0.0042  gm.  ZnO  at  18°,  conductivity 

method.  (Dupre  and  Bratas  —  Z.  angew.  Chem,  16,  55,  '03.) 

SOLUBILITY  OF  ZINC  HYDROXIDE  IN  ONE  PER  CENT  AQUEOUS 
SALT  SOLUTIONS  AT  i6°-2o°. 

(Snyder  —  Ber.  n,  936,  '78.) 

^  The  CO2  free  Zn(OH)2  dissolved  is  calculated  as  milligrams  Zn  per 
liter  of  the  given  salt  solution.  Additional  determinations  are  also 
given. 


Aq.  Salt       Mgs.  Zn  per 
Solution.    Liter  Solution. 

Aq.  Salt           Mgs.  Zn  per 
Solution.        Liter  Solution. 

Aq.  Salt          Mgs.  Zn  per 
Solution.        Liter  Solution. 

NaCl 

51 

K2S04 

37-5 

K2C03 

0 

KC1 

43 

MgS04 

27 

NH4C1 

95 

CaCl2 

57-5 

KNO3 

J7-5 

NH4N03 

77 

MgCl2 

65 

Ba(N03)2 

25 

(NH4)2S04 

88 

BaCl2 

38 

ZINC    HYDROXIDE 


SOLUBILITY  OF  ZINC  HYDROXIDE  IN  AQUEOUS  SOLUTIONS  OF: 


Ammonia  and  Ammonia  Bases 
at  i7°-i9°. 

(Herz  —  Z.  anorg.  Chem.  30,  281,  '02.) 

Sodium  Hydroxide  at 
Ord.  Temp. 

(Rubenbauer  —  Ibid.  30,  333,  '02.) 

Normality 
of 

Normality 
of  Dis- 

Gms. ZnO 
per  20  cc 

Gms.  per  20  cc.  Solution 

Mol. 
Dilution  of 

the  Base. 

solved  Zn. 

Solution. 

Na. 

Zn. 

the  NaOH. 

0 

>NH 

3 

0 

.0011 

0 

.00185 

o 

.1012 

0.0040 

4-50 

0 

236 

« 

O 

OIIO 

O 

.0180 

O 

,1978 

0.0150 

2-33 

O 

707 

ti 

o 

•059 

o 

.0958 

o 

.4278 

0.0442 

1.  06 

0 

,0944NH2CH3 

0 

.0005 

O 

.0008 

0 

.6670 

0.1771 

0.70 

0 

.472 

« 

0 

.0081 

0 

.0132 

0.9660 

0.9630 

0.48 

o 

944 

u 

o 

•03 

o 

.0484 

I 

•4951 

0.2481 

0.31 

o 

.068 

NH2C2H5 

o 

.0003 

o 

.0005 

2 

.9901 

0.3700 

0.16 

o 

•51 

« 

0 

.0045 

o 

.0074 

Moist  Zn 

(OH)  ,  used.     So- 

0 

.68 

« 

0 

.0098 

0 

.0161 

lutions 

shaken  5 

hours. 

ZINC    IODATE    Zn(IOs),. 

100  gms.  H2O  dissolve  0.87  gm.  Zn(IO3)2  cold  and  1.31  gms.  hot. 

(Rammelsberg  —  Pogg.  Ann,  43,  665,  '38.) 

ZINC    IODIDE     ZnI2. 

SOLUBILITY  IN  WATER. 

(Dietz  —  Wiss.  Abh.  p.  t.  Reichanstalt  3,  432,  'oo;  see  also  Etard  —  Ann.  chim.  phys.  [7]  2,  526,  '94.) 

Gms.  ZnI2         Mols.  ZnI2 

per  100  Gms.  per  100  Mols.  Solid  Phase. 


Gms.  ZnI2     Mols.  ZnI2 
per  100  Gms.      per  100      Solid  Phase. 
Mols.  H20. 

ZnI2.2H20 


Solution. 

Mols.  H2 

—  10 

80.50 

23-3 

-  5 

80-77 

23-7 

0 

81.16 

24-3 

+  10 

82.06 

25.8 

22 

83.12 

27.8 

27 

89.52 

50-3 

Solution. 

H20. 

O 

8i.ii 

24.2 

18 

81.20 

24.4 

40 

81.66 

25-1 

60 

82-37 

26.4 

80 

83-05 

27-5 

100 

83.62 

28.7 

ZnI3 


Sp.  Gr.  of  sat.  solution  of  the  anhydrous  salt  at  18°  =  2.725. 
ioo  gms.  glycerine  dissolve  40  gms.  ZnI2  at  15.5°. 

ZINC    NITRATE    Zn(NO3)2. 

SOLUBILITY  IN  WATER. 

(Funk  —  Wiss.  Abh.  p.  t.  Reichanstalt,  3,  438,  'oo.) 

Gms.  Mols. 

Zn(N03)2per   ZnNO3  per       Solid 
*   •  ioo  Gms.  ioo  Phase. 

Solution.       Mols.  H2O. 

6.36  Zn(NO3)2.9H20  1 8 


-25 

40.12 

0-30 

-22-5 

40.75 

6-54 

—  20 

42-03 

6.89 

-18 

43-59 

7-34 

-18 

44-63 

7-67 

-15 

45.26 

7.86 

—  13 

45  -51 

7-94 

—  12 

45-75 

8.01 

O 

48.66 

9.01 

H-12-s 

52-0 

10.3 

Gms. 

Mols. 

t°. 

Zn(N03)2  per 
ioo  Gms. 

Zn(N03)2 

IOO 

per       Solid 

Phase. 

Solution. 

Mols.  H20. 

18 

53-50 

IO-9 

Zn(NO3)a.6H20 

25 

55-90 

12.0 

" 

36 

4      63.63 

I6.7 

" 

36 

64.63 

17.4 

" 

5      65.83 

18.3 

" 

37 

66.38 

18.8 

Zn(NOa)3.3H,0 

40 

67.42 

19.7 

" 

41 

68.21 

20.4 

" 

43 

69.26 

21.4 

" 

45 

•5      77-77 

33-3 

M 

ZING    OXALATE  352 

ZINC    OXALATE    ZnC2O4.2H2O. 

One  liter  of   water  dissolve  0.083  M£-  equiv.  =  0.0064  gm.  ZnC2O4 
at  1 8°. 

(Kohlrausch  —  Z.  physik.  Chem.  50,  356,  '04- '05.) 

ZINC    SULPHATE    ZnSO4. 

SOLUBILITY  IN  WATER. 

(Cohen  —  Z.  physik.  Chem.  34,  189,  'oo;  at  50°;  Callender  and  Barnes  —  Proc.  Roy.  Soc.  62,  149,  '97; 
Etard  —  Ann.  chim.  phys.  [7]  2,  536,  '94;  Poggiale  Ibid.  [3]  8,  467,  '43;  Mulder.) 


1 

t  °. 

Gms.  ZnSO4>per  100  Gms.         Solid             *  0 

Gms.  ZnSO4  per  100 

Gms.           Solid 

Solution. 

Water. 

Phase. 

Solution. 

Water. 

Phase. 

-  5 

28 

.21 

39-30 

ZnSO4.7H2O       25 

38 

•94 

63 

•74 

ZnS04.6H2O 

O.I 

29 

•54 

41 

•93 

39 

41 

.22 

70 

.06 

.6H20  +  . 

7H20 

9.1 

32 

.01 

47 

.09 

50 

43 

•45 

76 

.84 

ZnS04.6H2O 

15 

33 

.81 

50 

.88 

70 

47 

•5 

88 

•7 

.6H20  + 

.H20 

25 

36 

.67 

57 

.90 

80 

46 

•4 

86 

.6 

ZnSCvHzO 

35 

39 

.98 

66 

.61 

90 

45 

•5 

83 

•7 

" 

39 

41 

.21 

7° 

•05 

IOO 

44 

•7 

80 

.8 

" 

-  5 

32 

•  OO 

47 

.08 

ZnS04.6H20    120 

41 

•7 

71 

•5 

• 

01 

33-09 

49 

.48 

I4O 

38 

.0 

61 

•3 

" 

160 

33-o 

49 

•3 

" 

zoo  gms.  abs.  methyl  alcohol  dissolve  0.65  gm.  ZnSO4  at  18°,  5.90 
gms.  ZnSO4.7H2O  at  18°. 

100  gms.  50  per  cent  methyl  alcohol  dissolve  15.7  gms.  ZnSO.7H2O 
at  1 8°. 

(de  Bruyn  —  Z.  physik.  Chem.  10,  783,  '92.) 


SOLUBILITY  OF  ZINC  SULPHATE  IN  AQUEOUS  ETHYL  ALCOHOL. 

(Schiff  —  Liebig's  Ann.  118,  365,  '61.) 

Concentration  of  Alcohol  10  per  cent     20  per  cent     40  per  cent 

Gms.  ZnSO4.7H2O  per  100 

Gms.  Solution  51.1  39 -o  3-45 

100  gms.  glycerine  dissolve  35  gms.  zinc  sulphate  at  15.5°. 


353 


ZINO    SULPHAT5 


SOLUBILITY  OF  ZINC  SULPHATE  —  SODIUM  SULPHATE  MIXTURES 

IN  WATER. 

(Koppel  —  Gumpery  —  Z.  physik.  Chem.  52,  409,  '05.) 


to 

Gms.  per  ioo 
Gms.  Solution. 

Gms.  per  ioo 
Gms.  H2O. 

Mols.  per  ioo 
Mols.  H20.                   Solid 

. 

ZnSO4. 

Na2SO4. 

ZnSO4 

Na2S04. 

ZnSO4. 

Na2S04: 

O 

27.19 

5-33 

40.30 

7.90 

4-50 

1.  01 

ZnSO^HzO  + 

5 

6.27 

42.28 

9-52 

4.71 

1.  2  1        )      Na2S04.ioH20 

25 

I7-58 

15-63 

26.32 

23.40 

2.94 

2.96        ZnNa2(S04)24H20 

30 

17.66 

15-58 

26.47 

23-44 

2-95 

2-97 

35 

J7-59 

15-70 

26.36 

23  -52 

2.94 

2.98 

40 

17-75 

15-72 

26.68 

23  .63 

2.98 

2.99 

10 

29.16 

7.16 

45-79 

ii  .24 

5-" 

1.42       ' 

15 

30.70 

6.40 

48.81 

10.17 

5-45 

1.29 

20 

32-51 

5-36 

52-34 

8.62 

5-84 

1.09 

ZnNa2(SO4)2  4H2O 

25 

34.36 

4.41 

56-15 

7.22 

6.27 

0.91 

-fZnSO/.yHzO 

30 

36.28 

3.80 

60.55 

6-34 

6.76 

0.81 

35 

38.18 

3-30 

65-25 

5-64 

7.28 

0.71     , 

38 

38-83 

2  .90 

66.64 

4.98 

7-44 

0-63     , 

ZnNa2(SO4)2  4HzO 

40 

38.26 

2.78 

64.89 

4.71 

7.24 

0.60 

+ZnSO4.6H2O 

10 

27.91 

7.92 

43-50 

12.34 

4-85 

I-565 

15 

24.28 

10.90 

36.92 

16.71 

4.12 

2  .  12 

20 

19.14 

14-58 

28.77 

21.95 

3.21 

2-79 

ZnNa2(S04)2^H20 
+Na2SO4.ioH2O 

25 

13  .31 

19.94 

19.93 

29.87 

2  .22 

3  -785 

30 

6.96 

27-75 

10.67 

42.51 

I  .19 

5-39     . 

35 

5-6i 

30.03 

8.72 

46.61 

0.971 

5.91        )  ZnNa2(S04)2.4H20 

40 

5-96 

28.65 

9.16 

43-83 

I  .02 

5-555   1   +Na2S°* 

ZINC    SULPHITE     ZnSO3.2H2O. 

100  gms.  H2O  dissolve  0.16  gm.  ZnSO4.2H2O. 

(Houston  and  Trichborne  —  Brit.  Med.  Jour.  1063,  '90. 


ZINC    TARTRATE  C4H4O6.Zn.2H2O. 

SOLUBILITY  IN  WATER. 

(Cantoni  and  Zachoder  —  Bull.  Soc.  chim.  [3]  33,  751,  '05.) 


Gms. 
t°.        CJt.06.Zn.2H2O 
per  100  cc.  Solution. 

15               0.019 
2O               O-022 
25               0.036 
30               0.041 

35          0.055 

Gms. 
t°.        C4H4Ob.Zn.2H20 
per  100  cc.  Solution. 

40          o  •  060 
45          0.073 

5O               0-087 

55          0.116 
60          o  .  104 

Gms. 
t°.      C4H406.Zn.2H2O 
per  100  cc.  Solution. 

65           o  .  ioo 

70               0.088 

75          0.078 
80          0.050 
85         0.041 

ZINC    VALERATE  (C4H9COO)2Zn.2H2O. 

ioo  gms.  H2O  dissolve  2  gms.  (C4H9COO)2.Zn.2H2O  at  25°. 
ioo  gms.  alcohol  dissolve  2.8  gms.  at  25°. 


(U.  S.  P.) 


ADDENDUM 

The  distribution  results  shown  in  the  following  table  were  obtained 
by  agitating  together  equal  volumes  of  olive  oil  and  aqueous  solutions 
of  the  several  narcotics,  and  determining  the  dissolved  substance 
present  in  the  aqueous  layer  before  and  after  the  agitation.  The  sum 
of  the  amount  of  substance  in  the  oil  and  aqueous  layers,  as  shown 
in  the  table,  is  the  amount  originally  in  100  cc.  of  each  aqueous  solu- 
tion used. 

The  work  was  done  for  the  purpose  of  testing  the  Overton-Meyer 
Theory  of  Narcosis,  that  the  anesthetic  action  of  certain  groups  of 
narcotics  is  proportional  to  their  distribution  between  water  and  the 
fatty  material  occurring  in  the  nervous  system,  and  olive  oil  was 
selected  as  the  solvent  best  fulfilling  the  analytical  requirements 
and  at  the  same  time  offering  a  fair  resemblance  to  the  fatty  substance 
of  the  nervous  system.  The  results  are  believed  to  be  of  interest 
both  as  solubility  studies  and  on  account  of  their  connection  with 
the  Theory  of  Narcosis. 

The  author  is  indebted  to  Dr.  Reid  Hunt  of  the  Hygienic  Laboratory 
for  calling  his  attention  to  the  papers  containing  the  distribution 
results  here  tabulated. 


354 


355 

DISTRIBUTION  OF  SEVERAL  SUBSTANCES  BETWEEN  WATER  AND 
OLIVE  OIL. 

(At  ord.  temp.,  Baum  —  Archiv.  exp.  Pathol-  u.  Pharmakol,  42,  130,  'go;  at  3°,  30°  and  36°;  Meyer  — 
Ibid.  46,  344,  '01;  at  15°,  Harrass —  Archh .  internal .  Pharmacodynamie  et  Therapie,  n,  458,  '03.) 


Name  of  Substance. 

Formula  . 

Gms.  Substance  per 

to                              100  CC. 

C(f.) 

Water 

Olive  Oil 

C(w.) 

layer  (w.). 

layer  (f.). 

Sulfonal 

(CH3)2C(S02.C2H6)2 

ord. 

0.0700 

0.0686 

o-979 

Trional 

(CH3)(C2H5)C(S02.C2H6)2 

it 

o  .  0404 

o.  1646 

4.074 

Tetronal 

(C2H6)2C(SO2.C2H5)2 

it 

0.0462 

o.  1446 

3.756 

Di  methyl  sulphon 

di  methyl  methane 

(CH3)2C(S02.CH3)2 

tt 

0.6072 

0.0622 

o.  103 

Di  ethyl  sulphon  me- 

thane 

CH2.(S02.C2H6)2 

" 

0.610 

0.092 

o.  151 

Ethyl  urethane 

NH2.C02.C2H5 

tt 

4-52 

0.6l5 

0.136 

Methyl  urethane 

NH2.C02.CH3 

" 

7-5° 

0.275 

0.037 

Tertiary  butyl  alcohol 

(CH3)2C(OH)CH3 

it 

8.744 

J-539 

o.  176 

Amylene  hydrate 

(CH3)2C(OH)CH2.CH3     . 

11 

6.605 

6.605 

I.  000 

Mono  acetin 

CaH6(OH)2.(OC2H30) 

ti 

4.28 

0.254 

0.059 

" 

" 

3 

2-349 

o.  229 

0.099 

n 

" 

36 

2.417 

0.161 

0.066 

Di  acetin 

CaH5(OH)(OC2H30)2 

ord. 

3-° 

°-7 

o.  234 

Tri  acetin 

C3H5(OC2H30)3 

2.72 

0.80 

0.205 

Bromal  hydrate 

CBr3CH(OH)2 

9.81 

6.52 

0.665 

Butyl  chloral  hydrate 

C3H4C13.CH(OH)2 

2.04 

3-24 

1.589 

Chloral  hydrate 

CCl3CH(OH)2 

16.31 

3.10 

o.  190 

.  " 

11 

4.12 

0.91 

0.22 

" 

•' 

3 

i-34 

0.08 

0-053 

n 

" 

30 

I-I5 

0.27 

0.237 

Salicylamide 

OH.C6H4.CH2NH2 

3 

0.056 

o.  126 

2.25 

" 

" 

36 

0.075 

0.107 

1.40 

Benzamide 

C7H6ONH2 

3 

1.062 

o.  706 

0.66 

" 

" 

36 

1.235 

0.533 

0-43 

Ethyl  alcohol 

C2H5OH 

3 

2.69 

0.09  ) 

0.026 

3 

3-90 

0.07  <) 

" 

" 

3° 

2.64 

o.  14  t 

f     / 

o.  047 

3° 

3.82 

o.  16  S 

Acetone 

(CH3)2CO 

3 

3-07 

°-5°i 

" 

3 

4.14 

0.52  > 

0.146 

" 

3 

3-92 

0.61  ) 

" 

3° 

2-73 

0-73) 

" 

3° 

3.86 

0.81  > 

0-235 

« 

3° 

0.87) 

Valeryl  di  ethyl  amide 

CH3(CH2)3CON(C3H6)2 

15 

0.231 

1-339 

5-797 

Valeryl  di  methyl  amide  CHa(CH2)3CON(CHa)2                1  5 

0.911 

0-379 

0.416 

Valeryl  ethyl  amide 

CH3(CH2)3CONH(C2Ha) 

15 

1.029 

0.261 

0.254 

Valer  amide 

CHa(CH2)aCONH2 

15 

0.769 

o.  241 

0-313 

Lactic  acid  di  ethyl 

amide 

CH3.CHOH.CON(C2H6)2 

15 

1.256 

0.194 

0.154 

Sodium  salicylate 

Q»H4.0H.COONa 

15 

1.444 

o.  156 

0.108 

INDEX 


Acenaphthene,  i. 
Acetamide,  i. 
Acetanilide,  i. 
Acetic  acid,  2-4. 

in  aq.  benzene,  55. 
Acetnaphthalide,  6. 
Acetone,  6-7,  355. 

in  aq.  benzene,  55. 

in  aq.  ethyl  acetate,  136. 

in  aq.  potassium  chlorate,  241. 

in  aq.  potassium  chloride,  247. 

in  aq.  potassium  nitrate,  258. 

in  aq.  sugar,  326. 
Acetphenetidine,  8. 
Acet-toluide,  8. 
Acetyl  acetone,  9. 
Acetylene,  8. 
Aconitine,  9. 
Adipic  acid,  9. 
Air,  10. 
Alanine,  10. 
Aldehyde,  n. 

propionic,  267. 
Alcohols,  ii,  355. 
Alcohol  in  aq.  benzene,  55. 

in  aq.  ether,  135. 

in  aq.  ethyl  acetate,  136. 

in  aq.  ethyl  butyrate,  136. 

in  aq.  ethyl  propionate,  136. 

in  aq.  ethyl  valerate,  137. 

in  aq.  methyl  butyrate,  204. 

in  aq.  propyl  acetate,  267 

in  aq.  potassium  carbonate,  239, 

in  aq.  potassium  chlorate,  241. 

in  aq.  potassium  nitrate,  258. 

in  aq.  sodium  carbonate,  297. 

in  aq.  sodium  nitrate,  308-9. 

in  aq.  sodium  sulphate,  314. 

in  aq.  sugar,  325. 
Allyl  isosulphocyanic  ester,  205. 
Aluminum  chloride,  12. 

rubidium  alum,  271. 

sulphate,  12. 

sulphate  +  Lithium  sulphate,  176. 

tellurium  alum,  332. 
Alums,  ammonium,  potassium,    etc., 

I3- 

caesium,  80. 

chromium,  116. 

iron  ammonium,  33. 

rubidium,  271. 

tellurium,  332. 
Amalgam,  278. 
Amido  benzoic  acids,  60. 

benzo  sulphonic  acids,  60. 


Amido  brom  benzo  sulphonic  acid,  57, 
nitro  benzoic  acids,  60. 

propionic  acid,  10. 

phenols,  60. 

Amines,  methyl,  etc.,  15-17. 
Ammonia,  17-19. 

lithium  sulphate,  water,  176. 
Ammonium  acid  formate,  26. 

acid  oxalate,  30. 

alum,  13. 

arsenate,  20. 

benzoate,  20. 

bicarbonate,  21-22. 

bicarbonate  -f  NaHCOa,  298. 

bichromate,  25. 

bromide,  20. 

bromide  +  KBr,  235. 

bromo  platinate,  20. 

cadmium  bromide,  20,  71. 

cadmium  chloride,  73. 

cadmium  iodides,  77. 

cadmium  sulphate,  33. 

carbonate,  21. 

carbonate  in  acetone,  6. 

cerium  nitrate,  111-112. 

cerium  sulphate,  112. 

chloride,  22-25. 

chloride  and  CuCl2,  125-126. 

chloride  and  KC1,  242. 

chloride  and  NaCl,  299-300. 

chloride  and  ZnCl2,  350. 

chromates,  25. 

chromium  sulphate,  33. 

cobalt  chlorides,  120. 

cobalt  sulphate,  33. 

copper  sulphate,  33,  129,  262. 

fluo  boride,  26. 

fluo  silicate,  31. 

formate,  26. 

iodate,  26. 

iodide,  26-28. 

iridium  sulphate,  34. 

iron  sulphate,  33. 

lead  cobalticyanide,  22. 

magnesium  nitrate,  30. 

magnesium  sulphate,  34. 

manganese  molybdate,  30. 

manganese  sulphate,  34. 

nickel  sulphate,  34,  129. 

nitrate,  24,  28,  30. 

oxalate,  30-31. 

permanganate,  31. 

persulphate,  35. 

phosphite,  31. 

platinic  chloride,  232-233. 


3.S7 


INDEX 


Ammonium  salicylate,  31. 

sodium  sulphate,  34. 

sodium  sulphite,  35. 

sulphate,  24,  31-33. 

sulphate  +  K2SO4,  261. 

sulphocyanide,  35. 

tetra  chromate,  25. 

tri  chromate,  25. 

tri  nitrate,  29. 

uranyl  carbonate,  22. 

uranyl  chlorides,  342. 

uranyl  nitrate,  343. 

uranyl  propionate,  343. 

vanadium  sulphate,  34. 

zinc  sulphate,  34,  129. 
Amyl  acetate,  35. 

alcohol,  ii. 

butyrate,  35. 

formate,  35. 

malonic  acid,  186. 

propionate,  35. 
Amylene  hydrate,  355. 
Anethol,  35. 

in  aq.  acetone,  6. 
Anilin,  36-38. 
Anis  acid,  38,  61. 
Anthracene,  39. 
Anthraquinone,  40. 
Antimony  potassium  tartrate,  41. 

tri  chloride,  40-41. 

tri  iodide,  41. 

Apo  morphine  hydrochloride,  205. 
Argon,  41. 
Arsenic  iodide,  41.         < 

pentoxide,  41. 

tri  iodide,  42. 
Asparagine,  42. 
Astrakanite,  312. 
Atropine,  42. 
Aurous,  auric,  see  Gold. 
Azelaic  acid,  43. 
Azo  phenetol,  43. 
Barium  acetate,  43. 

acid  oxalate,  52. 

arsenate,  43. 

bromate,  44. 

bromide,  44. 

butyrate,  44. 

cadmium  chloride,  74. 

caproate,  45. 

carbonate,  45. 

chlorate,  45. 

chloride,  24,  46-47. 

chloride  -f  NaCl,  300. 

chromate,  47. 

citrate,  47. 

cyanide,  48. 

dibrom,  etc.,  sulphonic  acid,  57. 

ferrocyanide,  48. 

fluoride,  48. 

formate,  48,  165. 

hydroxide,  48. 

iodate,  49. 


Barium  iodide,  49. 

iodide  +  BaBr2,  44. 

iodide  +  Hg(CN)2,  197, 

iso  caproate,  45. 

iso  succinate,  53. 

malate,  49. 

malonate,  49. 

molybdate,  49. 

nitrate,  24,  29,  50—51. 

nitrate  +  BaCl2,  46. 

nitrate  +  KNO3,  254. 

nitrite,  51. 

oxalate,  51. 

persulphate,  53. 

potassium  ferrocyanide,  48. 

propionate,  52. 

succinate,  53. 

sulphate,  52-53. 

tartrate,  53-54. 
Benzamide,  54,  355. 
Benzaldehyde,  54. 
Benzene,  54-56. 
Benzine,  58. 

Benzoic  acids,  58-62,  341. 
Benzoic  sulphinide,  62. 
Benzophenone,  6,  63. 
Benzo  sulphonic  acids,  57,  60. 
Benzoyl  phenyl  hydrazine,  57. 
Benzyl  carbamide,  104. 
Beryllium,  see  also  Glucinium. 
Beryllium  hydroxide,  63. 

salts,  140. 

sulphate,  63. 
Beta  Naphthol,  208. 
Borax,  293. 

Boric  acid,  65-67,  294. 
Boron  tri-fluoride,  67, 
Bismuth,  64. 

and  Pt  alloys,  232. 

chloride,  64. 

iodide,  64. 

nitrate,  64. 

oxide,  64. 

Bromal  hydrate,  355. 
Brom  benzene  (di),  56. 

benzoic  acid,  60. 

benzo  sulphonic  acid,  57. 

cinnamic  acid,  118. 

phenols,  226. 
Bromine,  67-69. 
Brucine,  69. 
Butane,  69. 
Butyl  acetate,  69. 

alcohol,  12. 

alcohol  tertiary,  355. 

chloral  hydrate,  355. 

formate,  69-70. 

malonic  acid,  186. 
Butyric  acid  (iso),  70. 

aldehyde,  69. 

Cadmium  ammonium  bromide,  20,  71. 
ammonium  chloride,  73. 
ammonium  iodides,  77. 


358 


INDEX 


Cadmium  ammonium  sulphate,  33. 

barium  chloride,  74. 

bromide,  70-71. 

caesium  sulphate,  84. 

chlorate,  72. 

cyanide,  76. 

fluoride,  77. 

hydroxide,  77. 

iodide,  77. 

magnesium  chloride,  74. 

nitrate,  78. 

oxalate,  78. 

potassium  bromide,  71. 

potassium  chloride,  76. 

potassium  iodide,  78. 

potassium  sulphate,  79. 

rubidium  bromide,  72. 

rubidium  chloride,  75. 

rubidium  sulphate,  274. 

sodium  bromide,  72. 

sodium  iodide,  78. 

sodium  sulphate,  80. 

sulphate,  78-79. 
Caesium  alums,  15,  80. 

cadmium  sulphate,  84. 

carbonate,  81. 

chloraurate,  Si. 

chloride,  81. 

chloride  +  FeCl3,  159. 

chlor  tellurate,  82. 

chromium  alum,  80. 

cobalt  sulphate,  84. 

copper  sulphate,  84. 

fluoboride,  81. 

gold  chloride,  141. 

iodate,  82. 

iodide,  82. 

indium  alum,  80. 

iron  alum,  80. 

iron  sulphate,  84. 

magnesium  sulphate,  84. 

manganese  sulphate,  84. 

mercuric  bromide,  81. 

nickel  sulphate,  84. 

nitrate,  82. 

oxalate,  83. 

permanganate,  83. 

platinic  chloride,  232. 

selenate,  83. 

sulphate,  83. 

tellurium  halides,  332. 

thallium  chloride,  82. 

uranyl  chloride,  342. 

uranyl  nitrate,  343. 

vanadium  alum,  80. 

zinc  sulphate,  84. 
Caffeine,  84. 
Calcium  acetate,  84-85. 

bicarbonate,  87-88. 

bitartrate,  103. 

bromide,  85. 

bromide  +  Hg(CN)2,  197. 

butyrate,  86. 


Calcium  caproate,  86. 

caprylate,  86. 

carbonate,  86. 

chlorate,  88. 

chloride,  88- -89. 

chromate,  90. 

citrate,  89. 

di  ethyl  acetate,  85. 

di  propyl  acetate,  85. 

fluoride,  90. 

formate,  90. 

heptoate,  91. 

hydroxide,  91. 

hydroxide  +  CaSO4,  99. 

iodate,  94. 

iodide,  94. 

iso  butyrate,  86. 

iso  butyl  acetate,  85. 

iso  succinate,  97. 

iso  valerate,  104. 

malate,  94. 

malonate,  94. 

methyl  ethyl  acetate,  85. 

methyl  pentanate,  86. 

methyl  propyl  acetate,  85. 

nitrate,  95. 

nonate,  96. 

oenanthate,  91. 

oxalate,  95. 

oxide,  91. 

pelargonate,  96. 

phosphates,  95-96. 

potassium  ferrocyanide,  90. 

potassium  sulphate,  101. 

propionate,  96. 

selenate,  97. 

silicate,  97. 

succinate,  97. 

sulphate,  97-102. 

sulphide,  1 02. 

sulphite,  103. 

tartrate,  103. 

tri  methyl  acetate,  85. 

valerate,  104. 
Camphoric  acid,  104. 
Cane  sugar,  324-326. 
Caoutchouc,  104. 
Carbamides,  104. 
Carbazole,  104. 
Carbon  bisulphide,  no. 

dioxide,  105-107. 

monoxide,  107-110. 

oxysulphide,  1 1 1 . 

tetra  chloride,  201. 
Carvoxime,  in. 
Cerium  acetate,  in. 

ammonium  nitrate,  iii-iia. 

ammonium  sulphate,  112. 

butyrate,  in. 

formate,  1 11. 

iso  butyrate,  in. 

propionate,  in. 

sulphate,  112. 
Chinin,  117. 
350 


INDEX 


Chiriidin,  117. 
Chlor  acetic  acid,  5. 
Chloral  hydrate,  113,  355. 

hydrate  butyl,  355. 
Chlor  benzene,  56. 

benzoic  acid,  60. 
Chlorine,  113-114. 

monoxide,  115. 

tri  oxide,  115. 
Chloroform,  115. 
Chlor  phenols,  226. 
Chromic  acid,  25,  116,  304. 
Chromium  alums,  116. 

ammonium  sulphate,  33. 

caesium  alum,  80. 

chloride,  116. 

double  salts,  116. 

potassium  cyanide,  250. 

potassium  molybdate,  116. 

rubidium  alum,  271. 

sulphate,  116. 

tellurium  alum,  332. 

tri  oxide,  25,  116,  304. 
Chrysarobin,  116. 
Chrysen,  117. 
Cinchona  alkaloids,  117. 

alkaloids  salts,  117. 
Cinnamic  acid,  118. 
Citric  acid,  119. 
Cobalt  ammonium  chlorides,  120. 

ammonium  sulphate,  33. 

bromide,  119. 

caesium  sulphate,  84. 

chlorate,  1.1.9. 

chloride,  120-121. 

double  salts,  119. 
Cobalticyanide  of  NH3  +  Pb,  22. 
Cobalt  iodate,  121. 

iodide,  121. 

lead  cyanide,  165. 

lead  potassium  cyanide,  165. 

nitrate,  121-122." 

potassium  sulphate,  262. 

rubidium  nitrite,  122. 

rubidium  sulphate,  274. 

sulphate,  122-123. 
Cocaine,  123. 

hydrochloride ,  1 2 3 . . 
Codeine,  123. 

salts,  123. 
Colchicine,  123. 
Collidin,  124. 
Copper  and  Pt  alloys,  232. 

acetate,  124. 

ammonium  chloride,  125-126. 

ammonium  sulphate,  33,  129. 

bromide,  124. 

caesium  sulphate,  84. 

chlorate,  124. 

chloride,  124-128. 

nitrate,  128. 

potassium  chloride,  127. 

potassium  sulphate,  131,  262. 


Copper  rubidium  sulphate,  274. 

sodium  sulphate,  131. 

sulphate,  32,  128-131. 

sulphate  +  CuCl2,  126. 

sulphate  +  MnSO4,  188. 

sulphate  +  NiSO4,  211. 

sulphide,  131. 

tartrate,  132. 

tellurium  sulphate,  334. 
Cream  of  tartar,  265-266. 
Cresol,  131. 

Cumidin  (pseudo),  132. 
Cuminic  acid,  132. 
Cuprous,  cupric,  see  Copper. 
Cyanogen,  132. 
Dextrose  in  aq.  acetone,  7. 
Di  acetin,  355. 
Di  brom  benzene,  56. 
Di  chlor  acetic  acid,  6. 
Didymium  potassium  sulphate,  133, 

sulphate,  133. 
Di  ethyl  amine,  16. 

ethyl  ketone,  137. 

ethyl  sulphone,  355. 
Di  methyl  sulphone,  355. 
Di  nitro  benzenes,  56—57. 

nitro  phenols,  226. 
Diphenyl,  227. 

phenyl  amine,  17. 
Erbium  sulphate,  133. 
Erythrite,  133. 
Ethane,  133. 
Ether,  134-135-  . 

in  anthraquinone,  40. 
Ethyl  acetate,  135-136. 

alcohol,  see  Alcohol. 

amines,  16. 

ammonium  bromide,  20. 

ammonium  chloride,  25. 

ammonium  iodide,  27, 

bromide,  137. 

butyrate,  136. 

carbamate,  138. 
Ethylene,  138. 

chloride,  137. 

cyanide,  323. 
Ethyl  formate,  136. 
Ethylidine  chloride,  137. 
Ethyl  iodide,  137. 

iso  valerate,  137. 

ketone,  137. 

malonic  acid,  186. 

methyl  ketone,  204. 

propionate,  136. 

urethane,  355. 

valerate,  137. 
Fats,  fatty  acids,  138. 
Ferrous,  ferric,  see  Iron. 
Ferri,  ferrocyanide  of  potassium,  250. 
Formaldehyde,  n. 
Fumaric  acid,  139. 
Furfurol,  139. 
Gadolinium  sulphate,  139. 


360 


INDEX 


Galactose,  139. 
Gallic  acid,  139, 
Germanium  dioxide,  140. 

potassium  fluoride,  251. 

sulphide,  140. 
Glass,  140. 

Glucinium,  see  also  Beryllium. 
Glucinium  hydroxide,  63. 

salts,  140. 

sulphate,  63. 
Glutaric  acid,  140. 
Glycolic  acid,  140. 
Gold,  140. 

alkali  chlorides,  140. 

caesium  chlorides,  81. 

chloride,  141. 

phosphorus  tri  chloride,  141. 
Grape  sugar,  325-326. 
Guaicol,  141. 

carbonate,  141. 
Guanidine,  141. 
Helium,  142. 
Hexane,  142. 
Hippuric  acid,  142. 
Homatropine,  hydrobromide,  143. 
Hydrastine,  143. 

chloride,  143. 
Hydrazine  sulphate,  143. 
Hydriodic  acid,  145. 
Hydrobromic  acid,  143. 
Hydrochloric  acid,  144. 
Hydrofluoric  acid,  145. 
Hydrogen,  145—149. 

sulphide,  150. 
Hydroquinone,  150-151. 
Hydroxy  benzoic  acids,  61. 
Hydroxylamine,  151. 

hydrochloride,  151. 
Hyoscyamine,  151. 
Hyoscine  hydrobromide,  151. 
Indium  ammonium  sulphate,  34. 

caesium  alum,  So. 
lodic  acid,  145. 
Iodine,  152—154. 
lodo  benzoic  acid,  60. 
Iron  ammonium  alum,  33. 

ammonium  sulphate,  33. 

caesium  alum,  So. 

caesium  sulphate,  84. 

chloride,  157—159. 

chloride  mix  crystals,  159. 

hydroxide,  160. 

lead  cyanide,  165. 

nitrate,  160. 

oxide,  1 60. 

phosphate,  160. 

potassium  sulphate,  161,  262. 

rubidium  alum,  271. 

rubidium  sulphate,  274. 

sulphate,  160. 

sulphate  +  CdSCK,  79. 

sulphate  +  Na2SO4,  161. 

sulphide,  160. 


Iron  tellurium  alum,  332. 

amyl  acetate,  35. 

amyl  alcohol,  1 1 . 

amyl  formate,  35. 

amyl  malonic  acid,  186. 
Iso  butyric  acid,  70. 

butyric  aldehyde,  69. 

butyl  acetate,  69-70. 

butyl  alcohol,  12. 

phtnalic  acid,  228. 

propyl  benzoic  acid,  132. 
Ketone,  di  ethyl,  137. 

methyl  ethyl,  204. 
Lactic  acid  di  ethyl  amide,  355. 
Lanthanum  bromate,  162. 

sulphate,  162. 
Lead,  162. 

and  Pt  alloys,  232. 

acetate,  162. 

ammonium     cobalticyanide, 
22. 

benzoate,  162. 

bromate,  162. 

bromide,  163. 

carbonate,  163. 

chlorate,  163. 

chloride,  163-165. 

chromate,  165. 

citrate,  165. 

cyanides,  165. 

fluoride,  165. 

formate,  165. 

hydroxide,  166. 

hyposulphate,  170. 

iodate,  166. 

iodide,  166-167. 

malate,  167. 

nitrate,  168. 

nitrate  +  BaCNO^,  50, 

oxalate,  168. 

oxides,  1 68. 

palmitate,  169. 

phosphate,  169. 

succinate,  169. 

sulphate,  169. 

tartrate,  170. 
Levulose,  170. 
Ligroin,  170. 

Lime,  see  Calcium  hydroxide, 
Lithium  benzoate,  170. 

bicarbonate,  172. 

bichromate,  173. 

borate,  170. 

bromate,  171. 

bromide,  171. 

carbonate,  171. 

chlorate,  172. 

chloraurate,  172. 

chloride,  172. 

chromate,  173. 

citrate,  173. 

fluoride,  173. 

formate,  174. 


INDEX 


Lithium  gold  chloride,  141. 

hydroxide,  174. 

hypophosphate,  176. 

iodate,  174. 

iodide,  175. 

laurinate,  176. 

myristate,  176. 

nitrate,  175. 

oleate,  176. 

oxalate,  175. 

palmitate,  176. 

permanganate,  176. 

phosphate,  176. 

stearate,  176. 

sulphate,  176. 
Magnesium  ammonium  nitrate,  30. 

ammonium  sulphate,  34. 

bicarbonate,  178-179. 

bromate,  177. 

bromide,  177. 

bromide  alcoholates,  177. 

bromide   aliphatic  compounds, 
177. 

bromide  etherates,  177. 

cadmium  chloride,  74. 

caesium  sulphate,  84. 

carbonate,  178-179. 

carbonate  in  aq.  acetone,  6. 

chlorate,  180. 

chloride,  180—181. 

chromate,  181. 

fluoride,  181. 

fluosilicate,  184. 

hydroxide,  181—182. 

hypophosphate,  184. 

iodate,  182. 

iodide,  182-183. 

iodide  alcoholate,  183. 

iodide,  alkyl  esters,  183. 

iodide,  aliphatic  compounds,  183. 

iodide  etherate,  183. 

nitrate,  184. 

oxalate,  184. 

platinic  chloride,  181. 

platinic  chromate,  181. 

potassium  sulphate,  185. 

salicylate,  184. 

sulphate,  184-185. 

sulphate  +  MgCl2,  181. 

sulphate  +  Na2SO4,  312. 

sulphite,  185. 
Maleic  acid,  139. 
Malonic  acid,  185—186. 
Maltose  in  aq.  acetone,  7. 
Manganese  ammonium  molybdate,3o. 

ammonium  sulphate,  34. 

borate,  186. 

bromide,  186. 

caesium  sulphate,  84. 

chloride,  187. 

fluo  silicate,  187. 

hypophosphate,  187. 

nitrate,  187. 


Manganese  potassium  vanadate,  189. 

sulphate,  188-189. 

sulphate  +  CuSO4,  130. 
Mannite,  189. 
Mannitol,  189. 
Mercury,  278. 

bromide,  189—190. 

caesium  bromide,  81. 

chloride  (ic),  190-196. 

chloride  (ous),  196. 

chloride  +  BaCl2,  46. 

chloride  +  CsCl,  81. 

cyanide,  197. 

fulminate,  197. 

iodide,  197—199. 

oxide,  200. 

sulphate,  200. 

tetra  methyl  amine  chloride,  195. 
Methane,  200. 
Methoxy  benzoic  acid,  38. 
Methyl  acetate,  203. 

alcohol,  136. 

amine,  15. 

amine  HgCl?,  195. 

ammonium  iodide,  26. 

benzoic  acids,  61,  341. 

butyrate,  203—204. 
Methylene  bromide,  203. 

chloride,  203. 
Methyl  ethyl  ketone,  204. 

iodide,  203. 

malonic  acid,  186. 

phenyl  carbamide,  104. 

propionate,  203. 

urethane,  355. 

valerate,  204. 
Milk  sugar,  325-326. 
Molybdenum  trioxide,  204. 
Monoacetin,  355. 
Mono  chlor  acetic  acid,  6. 
Morphine,  204-205. 

salts,  205. 
Mustard  oil,   205. 
Naphthalene,  206-207. 

in  aq.  acetone,  6. 
/S- Naphthalene  picrate,  55. 
Naphthoic  acid,  207. 
Naphthol,  208. 

Naphthylamine  sulphonic  acid,  206. 
Naphtion  acid,  206. 
Narceine,  208. 
Narcotics,  355. 
Neodymium  chloride,  208. 

sulphate,  208. 
Nickel  ammonium  sulphate,  34,  129. 

bromate,  208. 

bromide,  208. 

caesium  sulphate,  84. 

chloride,  208-209. 

iodate,  209. 

iodide,  209. 

nitrate,  210. 

potassium  sulphate,  212,  262. 


INDEX 


sulphate,  210-212. 

tellurium  sulphate,  334. 
Nicotine,  212. 

Nitranilines,  o,  m,  and  p,  38. 
Nitric  oxide,  218. 
Nitro  benzene,  56-57. 

benzoic  acids,  61-62. 
Nitrogen,  213-214. 
Nitrous  oxide,  215-218. 
Nitro  phenols,  226. 
Olive  oil  as  solvent,  355. 
Ortho  boric  acid,  65-67. 
Oxalic  acid,  31,  175,  219,  310. 
Oxygen,  220-221. 
Ozone,  221. 
Papaverine,  222. 
Paraffine,  222. 
Pentane  acid,  348. 
Pentanon,  137. 
Petroleum  benzine,  58. 
Phenacetine,  8. 
Phenanthrene,  222—223. 

picrate,  223. 
Phenic  acid,  223. 
Phenol,  223-225. 
Phenols  (amido),  60. 
Phenol  anilin  mixtures,  38. 
Phenolate  of  phenyl  ammonium,  226. 
Phenyl  ammonium,  phenolate,  226. 

amines,  17. 

di  amines,  226. 

guanidine  (tri),  141. 

hydrazine  (benzoyl),  57. 

methane  (tri),  201-203. 

salicylate,  227. 

thio  carbamide,  344-346. 

thio  urea,  344—346. 
Philocarpine  salts,  231. 
Phosphorus,  227-228. 
Phosphomolybdic  acid,  227. 
Phthalic  acids,  228. 

anhydride,  228—229. 
Physostigmine  salts,  229. 
Picric  acid,  229-231. 
Piperine,  231. 
Platino  amines,  233. 
Platinum  alloys,  232. 

ammonium  bromide,  20. 

bromide,  232. 

double  chlorides,  232. 

potassium  bromide,  232. 
Plumbic,  see  Lead. 
Potassium  acetate,  233. 

acid  formate,  251. 

acid  nitrate,  257. 

acid  oxalate,  259. 

acid  sulphate,  264. 

alum,  13-14. 

antimony  tartrate,  41. 

arsenate  (di  hydrogen),  233. 

barium  ferrocyanide,  48. 

benzoate,  233. 

bicarbonate,  238-239. 

bitartrate,  265-266. 


Potassium  berates,  234. 
boride  (fluo),  234. 
bromate,  234-235. 
bromide,  2315-238. 
bromide  and  chloride,  242. 
bromide  +  Hg(CN)2,  197. 
butyrate,  238. 
cadmium  bromide,  71. 
cadmium  chloride,  76. 
cadmium  iodide,  78. 
cadmium  sulphate,  79. 
calcium  ferrocyanide,  90. 
carbonate,  238-239. 
carbonate  in  aq.  acetone,  6. 
carbonate  in  aq.  ammonia,  180 
carbonyl  ferrocyanide,  250. 
chlorate,  239-241. 


chlorate  +  T1C1O, 


335- 


chloride,  24,  241-248. 
chloride  +  BaCl2,  46. 
chloride  +  CaCl2,  89. 
chloride  +  FeCl3,  159. 
chloride  +  HgCl2,  191. 
chloride  +  Hg(CN)2,  197. 
chloride  +  KBr,  236. 
chloride  +  KNO3,  255. 
chloride  +  NaCl,  300. 
chloride  +  Na2SO4,  312. 
chromates,  248-249. 
chromates  +  K2SO4,  263. 
chromium  alum,  116. 
chromium  molybdate,  116. 
chromisulphocyanide,  250. 
chromoc  yanide,  250. 
cobalt  sulphate,  262. 
copper  chloride,  127. 
copper  sulphate,  131,  262. 
citrate,  249. 
cyanate,  249. 
cyanide,  249. 
di  chromate,  248-249. 
didymium  sulphate,  133. 
ferric yanide,  250. 
ferrocyanide,  250. 
ferrosulphate,  262. 
fluoride,  250. 
fluo  boride,  234. 
fluo  germanate,  251. 
fluo  titanate,  266. 
formate,  251. 
gold  chloride,  141. 
hippurate,  142. 
hydroxide,  251. 
hypophosphate,  260. 
hypophosphite,  260. 
iodate,  252. 
iodide,  252-253. 
iodide  and  bromide,  236. 
iodide  and  chloride,  243. 
iodide  and  PbI2.  167. 
iodide  and  Hg(CN)2,  197. 
iron  sulphate,  161. 
lead  cobaltic  yanide,  165. 


363 


INDEX 


Potassium  lead  ferricyanide,  165. 

magnesium  chloride,  181. 

magnesium  chromate,  181. 

magnesium  cyanide,  181. 

magnesium  sulphate,  185. 

manganese  vanadate,  189. 

mercuric  cyanide,  197. 

nickel  sulphate,  212,  262. 

nitrate,  24,  29,  254—258. 

nitrate  +  Ba.(NOJ2,  50. 

nitrate  +  KBr,  237. 

nitrate  +  KC1,  244. 

nitrate  +  NaCl,  300. 

nitrate  +  NaNO3,  308. 

nitrite,  254. 

oxalate,  258-259. 

perchlorate,  241. 

perchlorate  +  KMnO4,  260. 

persulphate,  264. 

permanganate,  259-260. 

phosphate,  260. 

phosphite,  260. 

phosphomolvbdate,  261. 

platinic  bromide,  232. 

platinic  chloride,  232-233. 

selinate,  261. 

sodium  carbonate,  239. 

sodium  sulphate,  263. 

sodium  sulphite,  264. 

sodium  thio  sulphate,  264. 

stannate,  261. 

sulphate,  24,  32,  261-264. 

sulphate  +  KC1,  245. 

sulphate  +  KNO3,  256. 

sulphate  +  NaCl,  300. 

sulphate  +  Na2SO4,  312. 

sulphocyanide,  265,  291. 

tartrate,  265-266. 

tellurium  bromide,  332. 

thio  cyanate,  291. 

tri  chromate,  249. 

uranyl  butyrate,  343. 

uranyl  carbonate,  239. 

uranyl  chloride,  342. 

uranyl  nitrate,  343. 

uranyl  sulphate,  344. 

vanadate,  266. 

zinc  vanadate,  266. 
Praseodymium  sulphate,  267,, 
Propio  nitril,  267. 
Propionic  acid  (amido),  10. 

aldehyde,  267. 
Propylene,  268. 

Propyl  acetate,  butyrate,  etc.,  267- 
268. 

acetic  acid,  348. 

alcohol  in  aq.  K2CO3,  239. 

ammonium  iodide  (tetra),  28. 

anisol  (p),  35. 

bromide,  chloride,  etc.,  268. 

formate,  268. 

malonic  acid,  186. 
Pseudo  cumidin,  132. 


Pyrene,  268. 
Pyrogallol,  268. 
Pyrotartaric  acid,  140. 
Quinine  and  salts,  117,  269. 
Racemic  acid,  331. 
Resorcinol,  270 
Rhodium  salts,  270. 

sodium  nitrite,  309. 
Rubidium  alums,  15,  271. 

bromide,  271. 

brom  iodide,  273. 

cadmium  bromide,  72 

cadmium  chloride,  75. 

cadmium  sulphate,  274. 

carbonate,  271. 

chlorate,  271. 

chloride,  272. 

chromate,  272. 

cobalt  nitrate,  122. 

cobalt  sulphate,  274 

copper  sulphate,  274. 

di  chromate,  272. 

fluo  boride,  271. 

fluo  silicate,  273. 

gold  chloride,  141. 

hydroxide,  272. 

iodate,  272. 

iodide,  272-273. 

iron  sulphate,  274. 

nitrate,  273. 

mercuric  chlorides,  192. 

perchlorate,  271. 

permanganate,  273. 

permanganate  +  KMnO4,  260 

platinic  chloride,  232. 

selena te,  273. 

silico  tungstate,  273. 

sulphate,  273-274. 

tellurium  bromide,  332. 

tellurium  chloride,  272,  332 

thallium  chloride,  272. 

uranyl  chloride,  342. 

uranyl  nitrate,  343. 
Saccharine,  61. 
Salicylamid,  355. 
Salicylic  acid,  61,  274—276. 
Salol,  227. 
Selenious  acid,  277. 
Selenium,  276. 
Senfol,  205. 
Silicon,  277. 

Silico  tungstic  acid,  277. 
Silver,  278. 

and  Pt  alloys,  232. 

acetate,  278. 

benzoate,  279. 

borate,  279. 
bromate,  279-280. 
bromide,  280-281. 

butyrate,  281. 

caproates,  282. 

carbonate,  282. 

chlorate,  282. 


364 


INDEX 


Silver  chloride,  283-286, 

chromate,  286. 

citrate,  286. 

cyanide,  286. 

di  chromate,  286. 

di  ethyl  acetate,  279. 

di  propyl  acetate,  278. 

fluoride,  287. 

fulminate,  287. 

heptoate,  287. 

hydroxide  +  AgCl,  285. 

iodate,  287. 

iodide,  277,  287-288. 

iso  butyrate,  281. 

malate,  288. 

methyl  ethyl  acetate,  279. 

mono  chlor  acetate,  278. 

nitrate,  288-289. 

nitrate  +  KNO3,  257. 

nitrite,  289. 

onanthylate,  287. 

oxalate,  289. 

oxide,  289. 

permanganate,  289. 

phosphate,  289. 

propionate,  290. 

salicylate,  290. 

sodium  cyanide,  286. 

succinate,  290. 

sulphate,  290—291. 

sulphate  +  CaSO4,  101. 

sulphocyanide,  291. 

tartrate,  291. 

thallous  cyanide,  286. 

thio  cyanate,  291. 

tri  methyl  acetate,  279. 

valerates,  291—292. 

vanadate,  292. 
Sodium  acetate,  292—293. 

acid  formate,  305. 

alum,  15. 

ammonium  sulphate,  34. 

ammonium  sulphite,  35. 

arsenate,  293. 

benzoate,  293. 

bicarbonate,  22,  297—298. 

bicarbonate  +  NaCl,  300. 

bisulphate,  315. 

borate,  294. 

bromate,  294. 

bromide,  295. 

cadmium  bromide,  72. 

cadmium  iodide,  78. 

cadmium  sulphate,  80. 

carbonate,  296-297. 

carbonate  in  aq.  acetone,  6. 

chlorate,  298-299. 

chloride,  24,  299-303. 

chloride  +  BaCl2,  46. 

chloride  +  CaCl2,  89. 

chloride  +  FeCl3,  159. 

chloride  +  Hg(CN)2,  191. 

chloride  +  KC1,  245. 


Sodium  chloride  -f  KNO3,  256. 

chloride  +  Na2CO3,  298. 

chloride  +  NaClO3,  299. 

chromates,  303-304. 

citrate,  305. 

copper  sulphate,  131. 

ferrocyanide,  305. 

fluoride,  305. 

fluoride  phosphate,  310. 

fluo  silicate,  305. 

fluo  zirconate,  316. 

formate,  305. 

gold  chloride,  141. 

hydrogen  arsenate,  293. 

hydroxide,  306. 

hydroxide  +  NaCl,  301. 

hypophosphates,  311. 

hypophosphite,  311. 

iodate,  306. 

iodide,  306. 

iodide  +  Hg(CN)2,  197. 

mercuric  chloride,  193. 

mono  chromate,  303-304. 

molybdate,  307. 

nitrate,  29,  307-309. 

nitrate  +  KNO3,  256. 

nitrate  +  NaCl,  301. 

nitrate  +  AgNO3,  288. 

nitrite,  309. 

p  nitro  phenol,  310. 

oxalate,  309-310. 

phosphates,  310. 

phosphites,  311. 

potassium  carbonate,  239. 

potassium  sulphate,  263. 

potassium  sulphite,  264. 

potassium  thio  sulphate,  2640 

rhodonitrite,  309. 

salicylate,  275,  355. 

selinate,  311. 

silver  cyanide,  286. 

stannate,  311. 

sulphate,  311—315. 

sulphate  +  CoSO4,  122. 

sulphate  +  CuSO4,  131. 

sulphate  +  FeSO4.  161. 

sulphate  +  NiSO4,  2ir. 

sulphate  +  ZnSO4,  353. 

sulphite,  315. 

telluriate,  315. 

tetra  borate,  293. 

tetra  chromate,  304. 

thio  sulphate,  315. 

tri  molybdate,  307. 

tungstate,  316. 

uranyl  chromate,  343. 

wolfromate,  316. 
Stannous,  stannic,  see  Tin. 
Strontium  benzoate,  316. 

bicarbonate,  316. 

bromate,  316. 

bromide,  316. 

carbonate,  316. 


365 


INDEX 


Strontium  chlorate,  317. 
chloride,  317. 
chromate,  318. 
di  tungstate,  321. 
fluoride,  318. 
hydroxide,  318. 
hyposulphate,  170. 
iodate,  318. 
iodide,  318. 

iodide  +  Hg(CN)2,  197. 
malate,  319. 
molybdate,  319. 
nitrate,  319. 

nitrate  -f  Pb(NO3)2,  168. 
oxalate,  319. 
salicylate,  319. 
sulphate,  320. 
tartrate,  320—321. 
tungstate  (di),  321. 
Strychnine  and  salts,  321. 
Suberic  acid,  321. 
Succinic  acid,  322-323. 
anhydride,  322. 
nitril,  323. 
Succinimid,  323. 
Sugar,  324-326. 

in  aq.  acetone,  7. 
+  K.  Butyrate,  238. 
+  MgS04,  185. 
Sulphanilic  acid,  326. 
Sulphonal,  355. 
Sulphonic  acids,  57. 
Sulphur,  327—328. 
in  anilin,  36. 
in  benzene,  56. 
dioxide,  329-331. 
trioxide,  HgO  and  H2O,  200. 
Syngenite,  101. 
Tannic  acid,  331. 
Tartar  emetic,  41. 
Tartaric  acid,  331. 
Telluric  acid,  332. 
Tellurium,  331. 

caesium  bromide,  332. 
caesium  chloride,  82,  332. 
chromium  alum,  116. 
mercuric  cyanide,  197. 
potassium  bromide,  332. 
rubidium  bromide,  332. 
rubidium  chloride,  272,  332. 
Terephthalic  acid,  228. 
Tetra  boric  acid,  67. 
chlor  methane,  201. 
ethyl  ammonium  bromide,  20. 
ethyl  ammonium  chloride,  25. 
ethyl  ammonium  iodide,  27. 
methyl  ammonium  iodide,  26.  *. 
propyl  ammonium  iodide,  28. 
sodium  chromate,  304. 
Tetronal,  355. 


Thallium  alum,  14,  15,  332. 

bromate,  332. 

bromide,  332. 

caesium  chloride,  82. 

carbonate,  338. 

chlorate,  333. 

chloride,  333~335. 

chromate,  335. 

copper  sulphate,  338. 

cyanide,  336. 

fluoride,  336. 

iodate,  336. 

iodide,  336. 

nickel  sulphate,  338. 

nitrate,  336. 

nitrate  +  KNO3,  257. 

oxalate,  336-337. 

perchlorate,  338. 

phosphate,  337. 

picrate,  337. 

platinic  chloride,  232. 

rubidium  chloride,  272. 

silver  cyanide,  286. 

sulphate,  338. 

sulphide,  338. 

sulphite,  339. 

sulphocyanide,  338. 

vanadates,  339. 

zinc  sulphate,  338. 
Thallous  tri  chromate,  335. 
Thallo  thallic  chloride,  335. 
Theobromine,  339. 
Thio  urea  (phenyl),  344-346. 
Thorium  selenate,  339. 

sulphate,  339. 
Tin  chloride,  340. 

hydroxide,  340. 

iodide,  340-341. 

sulphate,  341. 
Toluene,  341. 
Toluidine,  341-342. 
Toluyl  acids,  341. 
Tolyl  carbamide,  104. 
Tri  acetin,  355. 

brom  phenols,  226. 

chlor  phenols,  226. 

chlor  acetic  acid,  6. 

ethyl  amine,  16. 

methyl  amine,  15. 

nitro  benzene,  57. 

oxymethylene,  n. 

phenyl  amine,  17. 

phenyl  guanidine,  141. 

phenyl  methane,  201. 
Trional,  355. 
Tungsto  silicic  acid,  277. 
Uranyl  ammonium  carbonate,  22. 

ammonium  propionate,  343. 

chloride,  342. 


366 


• 


INDEX 


Uranyl  double  chlorides,  342. 

double  nitrates,  343. 

nitrate,  343. 

potassium  butyrate,  343. 

potassium  carbonate,  239. 

potassium  sulphate,  344. 

sodium  chr ornate,  343. 

sulphate,  344. 
Urea,  344-346. 
Urethane,  347. 
Uric  acid,  347. 
Valerianic  acid,  348. 
Valeramide,  etc.,  355. 
Vanadium  ammonium  sulphate,  34, 

caesium  alum,  80. 

rubidium  alum,  271. 

tellurium  alum,  332. 
Ytterbium  sulphate,  348. 
Yttrium  iodate,  348. 
Zinc  and  Pt  alloys,  232. 
Zinc  acetate,  348. 

ammonium  sulphate,  34,  129. 


Zinc  benzoate,  348. 
bromide,  348. 
caesium  sulphate,  84. 
carbonate,  349. 
chlorate,  349. 
chloride,  349-350. 
cyanide,  349. 
fluoride,  350. 
hydroxide,  350-351. 
iodate,  351. 
iodide,  351. 
nitrate,  351. 
oxalate,  352. 
potassium  sulphate,  262. 
potassium  vanadate,  266. 
sulphate,  352-353. 
sulphate  +  CuSO4,  130. 
sulphite,  353. 
tartrate,  353. 
tellurium  sulphate,  334. 
valerate,  353. 


367 


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—  Symbolic  Algebra.     (Science  Series  No.  73.) .  .                              i6mo,  o  50 

Campin,  F.     The  Construction  of  Iron  Roofs 8vo,  2  oo 

Carpenter,  F.  D.     Geographical  Surveying.     (Science  Series  No.  37.) .  i6mo, 

Carpenter,  R.  C.,  and  Diederichs,  H.     Internal  Combustion  Engines .  8vo,  *s  oo 


6       D.   VAN   NOSTRAND   COMPANY'S   SHORT  TITLE   CATALOG 

Carter,  E.  T.     Motive  Power  and  Gearing  for  Electrical  Machinery  .  .  8vc,  *5  oo 

Carter,  H.  A.     Ramie  (Rhea),  China  Grass i2mo,  *2  oo 

Carter,  H.  R.     Modern  Flax,  Hemp,  and  Jute  Spinning 8vo,  *3  oo 

Cathcart,  W.  L.     Machine  Design.     Part  I.  Fastenings 8vo,  *3  oo 

Cathcart,  W.  L.,  and  Chaffee,  J.  I.     Elements  of  Graphic  Statics 8vo,  *3  oo 

Caven,  R.  M.,  and  Lander,  G.  D.     Systematic  Inorganic  Chemistry.  i2mo,  *2  oo 

Chambers'  Mathematical  Tables .^T7 8vo,  i  75 

Charnock,  G.  F.     Workshop  Practice.     (Westminster  Series.).  .  .  .8vo  (In  Press.) 

Charpentier,  P.     Timber 8vo,  *6  oo 

Chatley,  H.     Principles  and  Designs  of  Aeroplanes.    (Science    Series.) 

No.  126.) i6mo,  o  50 

—  How  to  Use  Water  Power i2mo,  *i  oo 

Child,  C.  T.     The  How  and  Why  of  Electricity i2mo,  i  oo 

Christie,  W.  W.     Boiler- waters,  Scale,  Corrosion,  Foaming 8vo,  *3  oo 

Chimney  Design  and  Theory 8vo,  *3  oo 

—  Furnace  Draft.     (Science  Series  No.  123.) i6mo,  o  50 

Church's  Laboratory  Guide.     Rewritten  by  Edward  Kinch 8vo,  *2  50 

Clapperton,  G.     Practical  Papermaking 8vo,  2  50 

Clark,  C.  H.     Marine  Gas  Engines (In  Press.) 

Clark,  D.  K.     Rules,  Tables  and  Data  for  Mechanical  Engineers 8vo,  5  oo 

Fuel:  Its  Combustion  and  Economy i2mo,  i  50 

-  The  Mechanical  Engineer's  Pocketbook i6mo,  2  oo 

-  Tramways:  Their  Construction  and  Working 8vo,  7  50 

Clark,  J.  M.     New  System  of  Laying  Out  Railway  Turnouts i2mo,  i  oo 

Clausen-Thue,  W.     ABC  Telegraphic  Code.     Fourth  Edition i2mo,  *5  oo 

Fifth  Edition 8vo,  *7  oo 

-  The  A  i  Telegraphic  Code 8vo,  *7  50 

Cleemann,  T.  M.     The  Railroad  Engineer's  Practice i2mo,  *i  50 

Clerk,  D.,  and  Idell,  F.  E.     Theory  of  the  Gas  Engine.     (Science  Series 

No.  62.) i6mo,  o  50 

Clevenger,  S.  R.  Treatise  on  the  Method  of  Government  Surveying. 

i6mo,  morocco 2  50 

Clouth,  F.  Rubber,  Gutta-Percha,  and  Balata 8vo,  *5  oo 

Coffin,  J.  H.  C.  Navigation  and  Nautical  Astronomy i2mo,  *3  50 

Colburn,  Z.,  and  Thurston,  R.  H.  Steam  Boiler  Explosions.  (Science 

Series  No.  2.) i6mo,  o  50 

Cole,  R.  S.  Treatise  on  Photographic  Optics i2mo,  2  50 

Coles- Finch,  W.  Water,  Its  Origin  and  Use. : 8vo,  *5  oo 

Collins,  J.  E.  Useful  Alloys  and  Memoranda  for  Goldsmiths,  Jewelers. 

i6mo •  o  50 

Constantino,  E.  Marine  Engineers,  Their  Qualifications  and  Duties. .  8vo,  *2  oo 

Coombs,  H.  A.  Gear  Teeth.  (Science  Series  No.  120.) i6mo,  o  50 

Cooper,  W.  R.  Primary  Batteries 8vo,  *4  oo 

-  "  The  Electrician  "  Primers , 8vo,  *5  oo 

Copperthwaite,  W.  C.     Tunnel  Shields 4to,  *9  oo 

Corey,  H.  T.     Water  Supply  Engineering 8vo  (In  Press.) 

Corfield,  W.  H.     Dwelling  Houses.     (Science  Series  No.  50.) i6mo,  o  50 

—  Water  and  Water-Supply.     (Science  Series  No.  17.) i6mo,  o  50 

Cornwall,  H.  B.     Manual  of  Blow-pipe  Analysis 8vo,  *2  50 

Courtney,  C.  F.     Masonry  Dams 8vo,  3  50 

Cowell,  W.  B.     Pure  Air,  Ozone,  and  Water i2mo,  *2  oo 


D.  VAN  NOSTRAND  COMPANY'S  SHORT  TITLE   CATALOG        7 

Craig,  T.     Motion  of  a  Solid  in  a  Fuel.     (Science  Series  No.  49.) i6mo,  o  50 

-  Wave  and  Vortex  Motion.     (Science  Series  No.  43.) i6mo,  o  50 

Cramp,  W.     Continuous  Current'Machine  Design 8vo,  *2  50 

Crocker,  F.  B.     Electric  Lighting.     Two  Volumes.     8vo. 

Vol.    I.     The  Generating  Plant 3  oo 

Vol.  II.     Distributing  Systems  and  Lamps 3  oo 

Crocker,  F.  B.,  and  Arendt,  M.     Electric  Motors 8vo,  *2  50 

Crocker,  F.  B.,  and  Wheeler,  S.  S.     The  Management  of  Electrical  Ma- 
chinery  I2mo,  *j  oo 

Cross,  C.  F.,  Bevan,  E.  J.,  and  Sindall,  R.  W.     Wood  Pulp  and  Its  Applica- 
tions.    (Westminster  Series.) 8vo  (In  Press.) 

Crosskey,  L.  R.     Elementary  Perspective 8vo,  i  oo 

Crosskey,  L.  R.,  and  Thaw,  J.     Advanced  Perspective 8vo,  i  50 

Culley,  J.  L.     Theory  of  Arches.     (Science  Series  No.  87.) i6mo,  o  50 

Davenport,  C.     The  Book.     (Westminster  Series.) 8vo,  *2  oo 

Davies,  E.  H.     Machinery  for  Metalliferous  Mines 8vo,  8  oo 

Davies,  D.  C.     Metalliferous  Minerals  and  Mining 8vo,  5  oo 

—  Earthy  Minerals  and  Mining 8vo,  5  oo 

Davies,  F.  H.     Electric  Power  and  Traction 8vo,  *2  oo 

Dawson,  P.     Electric  Traction  on  Railways 8vo,  *9  oo 

Day,  C.     The  Indicator  and  Its  Diagrams i2mo,  *2  oo 

Deerr,  N.     Sugar  and  the  Sugar  Cane 8vo,  *3  oo 

Deite,  C.     Manual  of  Soapmaking.     Trans,  by  S.  T.  King 4to,  *5  oo 

De  la  Coux,  H.   The  Industrial  Uses  of  Water.   Trans,  by  A.  Morris .  .  8vo,  *4  50 

Del  Mar,  W.  A.     Electric  Power  Conductors 8vo,  *2  oo 

Denny,  G.  A.     Deep-level  Mines  of  the  Rand 4to,  *io  oo 

—  Diamond  Drilling  for  Gold *5  oo 

De  Roos,  J.  D.  C.     Linkages.     (Science  Series  No.  47.) i6mo,  o  50 

De  Varona,  A.     Sewer  Gases.     (Science  Series  No.  55.) i6mo,  o  50 

Derr,  W.  L.     Block  Signal  Operation Oblong  i2mo,  *i  50 

Desaint,  A.     Three  Hundred  Shades  and  How  to  Mix  Them 8vo,  *io  oo 

Dibdin,  W.  J.     Public  Lighting  by  Gas  and  Electricity 8vo,  *8  oo 

—  Purification  of  Sewage  and  Water 8vo,  6  50 

Dieterich,  K.     Analysis  of  Resins,  Balsams,  and  Gum  Resins 8vo,  *3  oo 

Dinger,  Lieut.  H.  C.     Care  and  Operation  of  Naval  Machinery izmo,  *2  oo 

Dixon,  D.  B.     Machinist's  and  Steam  Engineer's  Practical  Calculator. 

i6mo,  morocco,  i  25 

Doble,  W.  A.     Power  Plant  Construction  on  the  Pacific  Coast  (In  Press.) 
Dodd,  G.     Dictionary    of    Manufactures,    Mining,    Machinery,    and    the 

Industrial  Arts i2mo,  i  50 

Dorr,  B.  F.     The  Surveyor's  Guide  and  Pocket  Table-book. 

i6mo,  morocco,  2  oo 

Down,  P.  B.     Handy  Copper  Wire  Table i6mo,  *i  oo 

Draper,  C.  H.     Elementary  Text-book  of  Light,  Heat  and  Sound. . .  i2mo,  i  oo 

-  Heat  and  the  Principles  of  Thermo-dynamics i2mo,  i  50 

Duckwall,  E.  W.     Canning  and  Preserving  of  Food  Products 8vo,  *5  oo 

Dumesny,  P.,  and  Noyer,  J.     Wood  Products,  Distillates,  and  Extracts. 

8vo,  *4  50 
Duncan,  W.  G.,  and  Penman,  D.     The  Electrical  Equipment  of  Collieries. 

8vo,  *4  oo 


8        D.  VAN   NOSTRAND   COMPANY'S  SHORT  TITLE  CATALOG 

Duthie,  A.  L.     Decorative  Glass  Processes.     (Westminster  Series.).  .8vo,  *2  oo 

Dyson,  S.  S.     Practical  Testing  of  Raw  Materials 8vo,  *s  oo 

Eccles,  R.  G.,  and  Duckwall,  E.  W.     Food  Preservatives 8vo,  i  oo 

Paper '.', . .  1  o  50 

Eddy,  H.  T.     Researches  in  Graphical  Statics 8vo,  i  50 

—  Maximum  Stresses  under  Concentrated  Loads. 8vo,  i  50 

Edgcumbe,  K.     Industrial  Electrical  Measuring  Instruments 8vo,  *2  50 

Eissler,  M.     The  Metallurgy  of  Gold 8vo,  7  50 

—  The  Hydrometallurgy  of  Copper 8vo,  *4  50 

-  The  Metallurgy  of  Silver 8vo,  4  oo 

—  The  Metallurgy  of  Argentiferous  Lead 8vo,  5  oo 

—  Cyanide  Process  for  the  Extraction  of  Gold 8vo,  3  oo 

—  A  Handbook  on  Modern  Explosives 8vo,  5  oo 

Ekin,  T.  C.     Water  Pipe  and  Sewage  Discharge  Diagrams folio,  *3  oo 

Eliot,  C.  W.,  and  Storer,  F-  H.     Compendious  Manual  of  Qualitative 

Chemical  Analysis i2mo,  *i  25 

Elliot,  Major  G.  H.     European  Light-house  Systems 8vo,  5  oo 

Ennis,  Wm.  D.     Linseed  Oil  and  Other  Seed  Oils 8vo,  *4  oo 

—  Applied  Thermodynamics 8vo  *4  50 

Erfurt,  J.     Dyeing  of  Paper  Pulp.     Trans,  by  J.  Hubner 8vo,  *7  50 

Erskine-Murray,  J.     A  Handbook  of  Wireless  Telegraphy 8vo,  *3  50 

Evans,  C.  A.     Macadamized  Roads (In  Press.} 

Ewing,  A.  J.     Magnetic  Induction  in  Iron 8vo,  *4  oo 

Fairie,  J.     Notes  on  Lead  Ores i2mo,  *i  oo 

—  Notes  on  Pottery  Clays i2mo,  *i  50 

Fairley,  W.,  and  Andre,  Geo.  J.     Ventilation  of  Coal  Mines.     (Science 

Series  No.  58.) i6mo,  o  50 

Fairweather,  W.  C.     Foreign  and  Colonial  Patent  Laws 8vo,  *3  oo 

Fanning,  J.  T.     Hydraulic  and  Water-supply  Engineering 8vo,  *5  oo 

Fauth,  P.     The  Moon  in  Modern  Astronomy.     Trans,  by  J.  McCabe. 

8vo,  *2  oo. 

Fay,  I.  W.     The  Coal-tar  Colors 8vo  (In  Press.} 

Fernbach,  R.  L.     Glue  and  Gelatine 8vo,  *3  oo 

Fischer,  E.     The  Preparation  of  Organic  Compounds.     Trans,  by  R.  V. 

Stanford i2mo,  *i  25 

Fish,  J.  C.  L.     Lettering  of  Working  Drawings Oblong  8vo,  i  oo 

Fisher,  H.  K.  C.,  and  Darby,  W.  C.     Submarine  Cable  Testing 8vo,  *3  50 

Fiske,  Lieut.  B.  A.     Electricity  in  Theory  and  Practice 8vo,  2  50 

Fleischmann,  W.    The  Book  of  the  Dairy.  Trans,  by  C.  M.  Aikman.   8vo,  4  oo 
Fleming,  J.  A.     The  Alternate-current  Transformer.     Two  Volumes.    8vo. 

Vol.   I.     The  Induction  of  Electric  Currents *5  oo 

Vol.  II.     The  Utilization  of  Induced  Currents *5  oo 

—  Centenary  of  the  Electrical  Current 8vo,  *o  50 

—  Electric  Lamps  and  Electric  Lighting 8vo,  *3  oo 

—  Electrical  Laboratory  Notes  and  Forms 4to,  *$  oo 

—  A  Handbook  for  the  Electrical  Laboratory  and  Testing  Room.     Two 

Volumes 8vo,  each,  *5  oo 

Fluery,  H.     The  Calculus  Without  Limits  or  Infinitesimals.     Trans,  by 
C.  0.  Mailloux (In  Press.) 


IX   VAN   NOSTRAND   COMPANY'S  SHOllT  TITLE  CATALOG        0 

Flynn,  P.  J,     Flow  of  Water.     (Science  Series  No.  84.) i6mo,  o  50 

—  Hydraulic  Tables.     (Science  Series  No.  66.) i6mo,  o  50 

Foley,  N.     British  and  American  Customary  and  Metric  Measures .  .  folio,  *3  oo 
Foster,  H.  A.     Electrical  Engineers'  Pocket-book.     (Sixth  Edition.) 

i2mo,  leather,  5  oo 

Foster,  Gen.  J.  G.     Submarine  Blasting  in  Boston  (Mass.)  Harbor 4to,  3  50 

Fowle,  F.  F.     Overhead  Transmission  Line  Crossings izmo,  *i  50 

-  The  Solution  of  Alternating  Current  Problems 8vo  (In  Press.) 

Fox,  W.  G.     Transition  Curves.     (Science  Series  No.  no.) i6mo,  o  50 

Fox,  W.,  and  Thomas,  C.  W.     Practical  Course  in  Mechanical  Draw- 
ing. .                                              I2mo,  i  25 

Foye,  J.  C.     Chemical  Problems.     (Science  Series  No.  69.) i6mo,  o  50 

—  Handbook  of  Mineralogy.     (Science  Series  No.  86.) i6mo,  o  50 

Francis,  J.  B.     Lowell  Hydraulic  Experiments 4to,  15  oo 

Frye,  A.  I.     Civil  Engineers'  Pocket-book (In  Press.) 

Fuller,  G.  W.     Investigations  into  the  Purification  of  the  Ohio  River. 4to,  *io  oo 

Furnell,  J.     Paints,  Colors,  Oils,  and  Varnishes 8vo,  *i  oo 

Gant,  L.  W.     Elements  of  Electric  Traction 8vo,  *2  50 

Garcke,  E.,  and  Fells,  J.  M.     Factory  Accounts 8vo,  3  oo 

Garforth,  W.  E.     Rules  for  Recovering  Coal  Mines  after  Explosions  and 

Fires i2mo,  leather,  i  50 

Gaudard,  J.     Foundations.     (Science  Series  No.  34.) i6mo,  o  50 

Gear,  H.  B.,  and  Williams,  P.  F.     Electric  Central  Station  Distributing 

Systems 8vo  (In  Preparation.) 

Geerligs,  H.  C.  P.     Cane  Sugar  and  Its  Manufacture 8vo,  *5  oo 

Geikie,  J.     Structural  and  Field  Geology 8vo,  *4  oo 

Gerber,  N.    Analysis  of  Milk,  Condensed  Milk,  and  Infants' Milk-Food.    8vo,  i  25 
Gerhard,  W.  P.     Sanitation,  Watersupply  and  Sewage  Disposal  of  Country 

Houses i2mo,  *2  oo 

—  Gas  Lighting.     (Science  Series  No.  in.) i6mo,  o  50 

—  Household  Wastes.     (Science  Series  No.  97.) i6mo,  o  50 

—  House  Drainage.     (Science  Series  No.  63.) i6mo,  o  50 

—  Sanitary  Drainage  of  Buildings.     (Science  Series  No.  93.) ....  i6mo,  o  50 

Gerhardi,  C.  W.  H.     Electricity  Meters 8vo,  *4  oo 

Geschwind,    L.     Manufacture    of    Alum   and   Sulphates.     Trans,    by   C. 

Salter 8vo,  *s  oo 

Gibbs,  W.  E.     Lighting  by  Acetylene i2mo,  *i  50 

-  Physics  of  Solids  and  Fluids.     (Carnegie  Technical  School's  Text- 

books.)   *i  50 

Gibson,  A.  H.     Hydraulics  and  Its  Application .  .                                      8vo,  *$  oo 

-  Water  Hammer  in  Hydraulic  Pipe  Lines I2mo,  *2  oo 

Gilbreth,  F.  B.     Motion  Study •  •  i2mo,  *2  oo 

Gillmore,  Gen.  Q.  A.     Limes,  Hydraulic  Cements  and  Mortars .  .             8vo,  4  oo 

-  Roads,  Streets,  and  Pavements i2mo,  2  oo 

Golding,  H.  A.     The  Theta-Phi  Diagram.. .                                            I2mo,  *i  25 

Goldschmidt,  R.     Alternating  Current  Commutator  Motor . .                 8vo,  *3  oo 

Goodchild,  W.     Precious  Stones.     (Westminster  Series.). .                  .8vo,  *2  oo 

Goodeve,  T.  M.     Textbook  on  the  Steam-engine. .                               i2mo,  2  oo 

Gore,  G.     Electrolytic  Separation  of  Metals 8vo,  *3  50 

Gould,  E.  S.     Arithmetic  of  the  Steam-engine i2mo,  i  oo 


10     D.  VAN  NOSTRAND  COMPANY'S  SHORT  TITLE  CATALOG 

Gould,  E.  S,      Calculus.     (Science  Series  No.  112.) i6mo,  o  50 

—  High  Masonry  Dams.     (Science  Series  No.  22.) i6mo,  o  50 

—  Practical  Hydrostatics  and  Hydrostatic   Formulas.     (Science  Series 

No.  117.) i6mo,  o  50 

Grant,  J.     Brewing  and  Distilling.     (Westminster  Series.)  8vo  (In  Press.) 

Gray,  J.     Electrical  Influence  Machines i2mo,  2  oo 

Greenwood,  E.     Classified  Guide  to  Technical  and  Commercial  Books.  8vo,  *3  oo 

Gregorius,  R.     Mineral  Waxes.     Trans,  by  C.  Salter i2mo,  *3  oo 

Griffiths,  A.  B.     A  Treatise  on  Manures i2mo,  3  oo 

—  Dental  Metallurgy 8vo,  *3  50 

Gross,  E.     Hops 8vo,  *4  50 

Grossman,  J.     Ammonia  and  Its  Compounds i2ino,  *i  25 

Groth,  L.  A.     Welding  and  Cutting  Metals  by  Gases  or  Electricity ....  8vo,  *3  oo 

Grover,  F.     Modern  Gas  and  Oil  Engines 8vo,  *2  oo 

Gruner,  A.     Power-loom  Weaving 8vo,  *3  oo 

Guldner,  Hugo.     Internal  Combustion  Engines.     Trans,  by  H.  Diederichs. 

4to,  *io  oo 

Gunther,  C.  O.     Integration i2mo,  *i  25 

Gurden,  R.  L.     Traverse  Tables folio,  half  morocco,  7  50 

Guy,  A.  E.     Experiments  on  the  Flexure  of  Beams 8vo,  *i  25 

Haeder,    H.      Handbook   on    the    Steam-engine.      Trans,  by  H.  H.  P. 

Powles i2mo,  3  oo 

Hainbach,  R.     Pottery  Decoration.     Trans,  by  C.  Slater i2mo,  *3  oo 

Hale,  W.  J.     Calculations  of  General  Chemistry i2mo,  *i  oo 

Hall,  C.  H.     Chemistry  of  Paints  and  Paint  Vehicles I2mo,  *2  oo 

Hall,  R.  H.     Governors  and  Governing  Mechanism i2mo,  *2  oo 

Hall,  W.  S.     Elements  of  the  Differential  and  Integral  Calculus 8vo,  *2  25 

—  Descriptive  Geometry 8vo  volume  and  a  4to  atlas,  *3  50 

Haller,  G.  F.,  and  Cunningham,  E.  T.     The  Tesla  Coil , i2mo,  *i  25 

Halsey,  F.  A.     Slide  Valve  Gears i2mo,  i  50 

-  The  Use  of  the  Slide  Rule.     (Science  Series  No.  114.) i6mo,  o  50 

—  Worm  and  Spiral  Gearing.     (Science  Series  No.  116.) i6mo,  o  50 

Hamilton,  W.  G.     Useful  Information  for  Railway  Men i6mo,  i  oo 

Hammer,  W.  J.     Radium  and  Other  Radio-active  Substances 8vo,  *i  oo 

Hancock,  H.     Textbook  of  Mechanics  and  Hydrostatics 8vo,  i  50 

Hardy,  E.     Elementary  Principles  of  Graphic  Statics i2mo,  *i  50 

Harper,  W.  B.     Utilization  of  Wood  Waste  by  Distillation 4to,  *3  oo 

Harrison,  W.  B.     The  Mechanics'  Tool-book i2mo,  i  50 

Hart,  J.  W.     External  Plumbing  Work 8vo,  *3  oo 

—  Hints  to  Plumbers  on  Joint  Wiping 8vo,  *3  oo 

—  Principles  of  Hot  Water  Supply 8vo,  *3  oo 

Sanitary  Plumbing  and  Drainage 8vo,  *3  oo 

Haskins,  C.  H.     The  Galvanometer  and  Its  Uses i6mo,  i  50 

Hatt,  J.  A.  H.     The  Colorist square  i2mo,  *i  50 

Hausbrand,  E.     Drying  by  Means  of  Air  and  Steam.     Trans,  by  A.  C. 

Wright i2mo,  *2  oo 

—  Evaporating,  Condensing  and  Cooling  Apparatus.     Trans,  by  A.  C. 

Wright 8vo,  *5  oo 

Hausner,  A.     Manufacture  of  Preserved  Foods  and  Sweetmeats.     Trans. 

by  A.  Morris  and  H.  Robson : 8vo,  *3  oo 


D.   VAN   NOSTRAND   COMPANY'S   SHOUT  TITLE  CATALOG      11 

Hawke,  W.  H.     Premier  Cipher  Telegraphic  Code  ..............  4to,     *s  oo 

-  100,000  Words  Supplement  to  the  Premier  Code  .......  4to,     *s  oo 

Hawkesworth,  J.     Graphical  Handbook  for  Reinforced  Concrete  Design. 


4to,  *2  50 

Hay,  A.     Alternating  Currents  ................................  gVO)  *2  5O 

-  Principles  of  Alternate-current  Working  ........                      .  .  i2mo'  2  oo 

-  Electrical  Distributing  Networks  and  Distributing  Lines  ........  8vo,  *3  50 

—  Continuous  Current  Engineering  ............................  gVO)  *2  5O 

Heap,  Major  D.  P.     Electrical  Appliances  ...........                            .8vo,  2  oo 

Heaviside,  0.     Electromagnetic  Theory.     Two  Volumes.          ..8vo,  each,  *5  oo 
Heck,  R.  C.  H.     Steam-Engine  and  Other  Steam  Motors.     Two  Volumes. 

Vol.    I.     Thermodynamics  and  the  Mechanics  .................  8vo,  *3  50 

Vol.  II.     Form,  Construction,  and  Working  ...................  8vo,  *s  oo 

-  Abridged  edition  of  above  volumes  (Elementary)  .....  8vo  (In  Preparation.) 

—  Notes  on  Elementary  Kinematics  ...................  8vo,  boards,  *i  oo 

—  Graphics  of  Machine  Forces  .........................  8vo,  boards,  *i  oo 

Hedges,  K.     Modern  Lightning  Conductors  .......................  8vo,  3  oo 

Heermann,  P.     Dyers'  Materials.     Trans,  by  A.  C.  Wright  .........  i2mo,  *2  50 

Hellot,  Macquer  and  D'Apligny.     Art  of  Dyeing  Wool,  Silk  and  Cotton. 

8vo,  *2  oo 

Henrici,  0.     Skeleton  Structures  .................................  8vo,  i  50 

Hermann,  F.     Painting  on  Glass  and  Porcelain  ....................  8vo,  *3  50 

Herrmann,  G.     The  Graphical  Statics  of  Mechanism.     Trans,  by  A.  P. 

Smith  ..............................................  i2mo,  2  oo 

Herzfeld,  J.     Testing  of  Yarns  and  Textile  Fabrics  .................  8vo,  *3  50 

Hildebrandt,  A.     Airships,  Past  and  Present  .......................  8vo,  *3  50 

Hildenbrand,  B.  W.     Cable-Making.     (Science  Series  No.  32.)  .....  i6mo,  o  50 

Hill,  J.  W.     The  Purification  of  Public  Water  Supplies.      New  Edition.     (In  P/rs.s.) 

—  Interpretation  of  Water  Analysis  ......................  (In  Press.) 

Hiroi,  I.     Plate  Girder  Construction.     (Science  Series  No.  95.)  .....  i6mo,  o  50 

—  Statically-Indeterminate  Stresses  ..........................  i2mo,  *2  oo 

Hirshfeld,  C.  F.     Engineering  Thermodynamics.     (Science  Series  No.  45.) 

i6mo,  o  50 

Hobart,  H.  M.     Heavy  Electrical  Engineering  .....................  8vo,  *4  50 

—  Electricity  ...............................................  8vo,  *2  oo 

—  Electric  Trains  ...........................................  8vo,  *2  50 

Hobbs,  W.  R.  P.     The  Arithmetic  of  Electrical  Measurements  .....  i2mo,  o  50 

Hoff,  J.  N.     Paint  and  Varnish  Facts  and  Formulas  ..............  i2ino,  *i  50 

Hoff,  Com.  W.  B.     The  Avoidance  of  Collisions  at  Sea.  .  .  i6mo,  morocco,  o  75 

Hole,  W.     The  Distribution  of  Gas  ..............................  8vo,  *y  50 

Holley,  A.  L.     Railway  Practice  ..............................  folio,  12  oo 

Holmes,  A.  B.     The  Electric  Light  Popularly  Explained  ....  i2mo,  paper,  o  50 

Hopkins,  N.  M.     Experimental  Electrochemistry  .....                             8vo,  *3  oo 

-  Model  Engines  and  Small  Boats  ............                            .  .  12010,  i   25 

Hopkinson,  J.     Shoolbred,  J.  N.,  and  Day,  R.  E.     Dynamic   Electricity. 

(Science  Series  No.  71.)  .................                              i6mo,  050 

Horner,  J.     Engineers'  Turning  .....................                         8vo,  *3  50 

-  Metal  Turning  ................                                                    •    "mo,  i  50 

-  Toothed  Gearing  .......                                                                ..12010,  225 

Houghton,  C.  E.     The  Elements  of  Mechanics  of  Materials  ......  i2rno,  *2  oo 

Houllevique,  L.     The  Evolution  of  the  Sciences  ...................  8vo,  *2  oo 


12     D.   VAN   NOSTRAND  COMPANY'S  SHORT  TITLE   CATALOG 

Howe,  G.     Mathematics  for  the  Practical  Man i2mo,  *i  25 

Howorth,  J.     Repairing  and  Riveting  Glass,  China  and  Earthenware. 

8vo,  paper,  *o  50 

Hubbard,  E.     The  Utilization  of  Wood- waste 8vo,  *2  50 

Humber,  W.     Calculation  of  Strains  in  Girders i2mo,  2  50 

Humphreys,  A.  C.     The  Business  Features  of  Engineering  Practice.  .  8vo,  *i  25 

Hurst,  G.  H.     Handbook  of  the  Theory  of  Color 8vo,  *2  50 

—  Dictionary  of  Chemicals  and  Raw  Products 8vo,  *3  oo 

—  Lubricating  Oils,  Fats  and  Greases 8vo,  *3  oo 

—  Soaps : '..... '. 8vo,  *s  oo 

—  Textile  Soaps  and  Oils 8vo,  *2  50 

Hurst,  H.  E.,  and  Lattey,  R.  T.     Text-book  of  Physics. 8vo,  *3  oo 

Hutchinson  R.  W.,  Jr.     Long  Distance  Electric  Power  Transmission .  i2mo,  *3  oo 
Hutchinson,  R.  W.,  Jr.,  and  Ihlseng,  M.  C.     Electricity  in  Mining.  .  i2mo, 

(In  Press) 
Hutchinson,  W.  B.     Patents  and  How  to  Make  Money  Out  of  Them. 

i2mo,  i  25 

Hutton,  W.  S.     Steam-boiler  Construction 8vo,  6  oo 

—  Practical  Engineer's  Handbook '.' . '\ ','.  ' .' V 8vo,  7  oo 

—  The  Works'  Manager's  Handbook  •. 8vo,  6  oo 

Hyde,  E.  W.     Skew  Arches.     (Science  Series  No.  15.) i6mo,  o  50 

Induction  Coils.     (Science  Series  No.  53.) i6mo,  o  50 

Ingle,  H.     Manual  of  Agricultural  Chemistry  . 8vo,  *3  oo 

Innes,  C.  H.     Problems  in  Machine  Design i2mo,  *2  oo 

—  Air  Compressors  and  Blowing  Engines i2mo,  *2  oo 

—  Centrifugal  Pumps i2mo,  *2  oo 

—  The  Fan i2mo,  *2  oo 

Isherwood,  B.  F.     Engineering  Precedents  for  Steam  Machinery 8vo,  2  50 

Ivatts,  E.  B.     Railway  Management  at-Stations.. 8vo,  *2  50 

Jacob,  A.,  and  Gould,  E.   S.     On  the   Designing   and  Construction  of 

Storage  Reservoirs.     (Science  Series  No.  6.) i6mo,  o  50 

Jamieson,  A.     Text  Book  on  Steam  and  Steam  Engines 8vo,  3  oo 

—  Elementary  Manual  on  Steam  and  the  Steam  Engine i2mo,  i  50 

Jannettaz,  E.     Guide  to  the  Determination  of  Rocks.     Trans,  by  G.  W. 

Plympton i2mo,  i  50 

Jehl,  F.     Manufacture  of  Carbons: 8vo,  *4  oo 

Jennings,  A.  S.     Commercial  Paints  and  Painting.     (Westminster  Series.) 

8vo  (In  Press.) 

Jennison,  F.  H.     The  Manufacture  of  Lake  Pigments 8vo,  *3  oo 

Jepson,  G.     Cams  and  the  Principles  of  their  Construction 8vo,  *i   50 

—  Mechanical  Drawing 8vo  (In  Preparation.) 

Jockin,  W.     Arithmetic  of  the  Gold  and  Silversmith i2mo,  *i  oo 

Johnson,  G.  L.     Photographic  Optics  and  Color  Photography 8vo,  *3  oo 

Johnson,  W.  H.     The  Cultivation  and  Preparation  of  Para  Rubber. .  .8vo,  *3  oo 

Johnson,  W.  McA.     The  Metallurgy  of  Nickel (In  Preparation.) 

Johnston,  J.  F.  W.,  and  Cameron,  C.     Elements  of  Agricultural  Chemistry 

and  Geology i2mo,  2  60 

Joly,  J.     Raideactivity  and  Geology i2mo,  *3  oo 

Jones,  H.  C.     Electrical  Nature  of  Matter  and  Radioactivity i2mo,  *2  oq 


D.   VAN   NOSTRAND   COMPANY'S  SHORT  TITLE  CATALOG  13 

Jones,  M.  W.     Testing  Raw  Materials  Used  in  Paint i2mo,  *2  oo 

Jones,  L.,  and  Scard,  F.  I.     Manufacture  of  Cane  Sugar 8vo,  *5  oo 

Joy,  G.  A.,  and  Thiess,  J.  B.     Toll  Telephone  Practice.  .          .  .(In  Pres.s.) 

Joynson,  F.  H.     Designing  and  Construction  of  Machine  Gearing. .  .  .8vo,  2  oo 

Jiiptner,  H.  F.  V.     Siderology:  The  Science  of  Iron .  .8vo,  *5  oo 

Kansas  City  Bridge 4to,  6  oo 

Kapp,  G.     Alternate  Current  Machinery.     (Science  Series  No.  96.) .  i6mo,  c  50 

—  Dynamos,  Motors,  Alternators  and  Rotary  Converters.     Trans,  by 

H.  H.  Simmons 8vo,  4  oo 

—  Electric  Transmission  of  Energy i2mo,  3  50 

Keim,  A.  W.     Prevention  of  Dampness  in  Buildings 8vo,  *2  oo 

Keller,  S.  S.     Mathematics  for  Engineering  Students.     i2mo,  half  leather. 

Algebra  and  Trigonometry,  with  a  Chapter  on  Vectors *i  75 

Special  Algebra  Edition *i  oo 

Plane  and  Solid  Geometry *i  25 

Analytical  Geometry  and  Calculus *2  oo 

Kelsey,  W.  R.     Continuous-current  Dynamos  and  Motors 8vo,  *2  50 

Kemble,  W.  T.,  and  Underbill,  C.  R.     The  Periodic  Law  and  the  Hydrogen 

Spectrum 8vo,  paper,  *o  50 

Kemp,  J.  F.     Handbook  of  Rocks 8vo,  *i  50 

Kendall,  E.     Twelve  Figure  Cipher  Code 410,  *is  oo 

Kennedy,  A.  B.  W.,  and  Thurston,  R.  H.     Kinematics  of  Machinery. 

(Science  Series  No.  54.) i6mo,  o  50 

Kennedy,  A.  B.  W.,  Unwin,  W.  C.,  and  Idell,  F.  E.     Compressed  Air. 

(Science  Series  No.  106.) i6mo,  o  50 

Kennedy.  R.     Modern  Engines  and  Power  Generators.     Six  Volumes.   4to,  1500 

Single  Volumes each,  3  oo 

—  Electrical  Installations.     Five  Volumes 4to,  15  oo 

Single  Volumes each,  3  50 

—  Flying  Machines;  Practice  and  Design i2mo,  *2  oo 

Kennelly,  A.  E.     Electro-dynamic  Machinery 8vo,  i  50 

Kent,  W.     Strength  of  Materials. '    (Science  Series  No.  41.) i6mo,  o  50 

Kershaw,  J.  B.  C.     Fuel,  Water  and  Gas  Analysis 8vo,  *2  50 

—  Electrometallurgy.     (Westminster  Series.) 8vo,  *2  oo 

Kershaw,  J.  B.  C.     The  Electric  Furnace  in  Iron  and  Steel  Production. 

I2mo,  *i  50 

Kingdon,  J.  A.     Applied  Magnetism 8vo,  *3  oo 

Kinzbrunner,  C.     Alternate  Current  Windings 8vo,  *i  50 

—  Continuous  Current  Armatures 8vo,  *i  50 

-  Testing  of  Alternating  Current  Machines 8vo,  *2  oo 

Kirkaldy,  W.  G.     David  Kirkaldy's  System  of  Mechanical  Testing. . .  .4to,  10  oo 

Kirkbride,  J.     Engraving  for  Illustration .8vo,  *i  50 

Kirkwood,  J.  P.     Filtration  of  River  Waters 4*0,  7  5° 

Klein,  J.  F.     Design  of  a  High-speed  Steam-engine. .                            .8vo,  *5  oo 

—  Physical  Significance  of  Entropy 8vo,  *i  50 

Kleinhans,  F.  B.     Boiler  Construction ' 8vo,  3  oo 

Knight,  Lieut.-Com.  A.  M.     Modern  Seamanship 8vo,  *6  oo 

Half  morocco *7  5<> 

Knox,  W.  F.     Logarithm  Tables (In  Prcjxiratwn.) 

Knott,  C.  G.,  and  Mackay,  J.  S.     Practical  Mathematics 8vo,  2  oo 


14     D.  VAN   NOSTRAND   COMPANY'S  SHORT  TITLE   CATALOG 

Koester,  F.     Steam-Electric  Power  Plants 4to,  *s  oo 

—  Hydroelectric  Developments  and  Engineering 4to,  *5  oo 

Koller,  T.     The  Utilization  of  Waste  Products 8vo,  *3  50 

—  Cosmetics 8vo,  *2  50 

Krauch,  C.     Testing  of  Chemical  Reagents.     Trans,  by  J.  A.  Williamson 

and  L.  W.  Dupre 8vo,     *3  oo 

Lambert,  T.     Lead  and  its  Compounds 8vo,  *3  50 

—  Bone  Products  and  Manures 8vo,  *3  oo 

Lamborn,  L.  L.     Cottonseed  Products 8vo,  *3  oo 

—  Modern  Soaps,  Candles,  and  Glycerin 8vo,  *7  50 

Lamprecht,  R.     Recovery  Work  After  Pit  Fires.     Trans,  by  C.  Salter . .  8vo,  *4  oo 
Lanchester,  F.  W.     Aerial  Flight.     Two  Volumes.     8vo. 

Vol.    I.     Aerodynamics *6  oo 

Vol.  II.     Aerodonetics *6  oo 

Larner,  E.  T.     Principles  of  Alternating  Currents i2mo,  *i  25 

Larrabee,  C.  S.     Cipher  and  Secret  Letter  and  Telegraphic  Code i6mo,  o  60 

La  Rue,  B.  F.     Swing  Bridges.     (Science  Series  No.  107.) i6mo,  o  50 

Lassar-Cohn,  Dr.     Modern  Scientific  Chemistry.     Trans,  by  M.  M.  Patti- 

son  Muir i2mo,  *2  oo 

Latimer,  L.  H.,  Field,  C.  J.,  and  Howell,  J.  W.     Incandescent  Electric 

Lighting.     (Science  Series  No.  57.) i6mo,  o  50 

Latta,  M.  N.     Handbook  of  American  Gas-Engineering  Practice 8vo,  *4  50 

—  American  Producer  Gas  Practice 4to,  *6  oo 

Leask,  A.  R.     Breakdowns  at  Sea i2mo,  2  oo 

-  Triple  and  Quadruple  Expansion  Engines i2mo,  2  oo 

—  Refrigerating  Machinery I2mo,  2  oo 

Lecky,  S.  T.  S.     "  Wrinkles  "  in  Practical  Navigation 8vo,  *8  oo 

Le  Doux,  M.     Ice-Making  Machines.     (Science  Series  No.  46.) ....  i6mo,  o  50 

Leeds,  C.  C.     Mechanical  Drawing  for  Trade  Schools oblong  4to, 

High  School  Edition *i  25 

Machinery  Trades  Edition *2  oo 

Lefe"vre,  L.     Architectural  Pottery.      Trans,  by  H.  K.  Bird  and  W.  M. 

Binns 4to,     *7  50 

Lehner,  S.     Ink  Manufacture.     Trans,  by  A.  Morris  and  H.  Robson  . .  8vo,     *2  50 

Lemstrom,  S.     Electricity  in  Agriculture  and  Horticulture 8vo,     *i  ,50 

Le  Van,  W.  B.     Steam-Engine  Indicator.     (Science  Series  No.  78.) .  i6mo,       o  50 

Lewes,  V.  B.     Liquid  and  Gaseous  Fuels.     (Westminster  Series.). . .  .8vo,     *2  oo 

Lieber,  B.  F.     Lieber's  Standard  Telegraphic  Code 8vo,  *io  oo 

Code.     German  Edition 8vo,  *io  oo 

— -  Spanish  Edition 8vo,  *io  oo 

—  French  Edition 8vo,  *io  oo 

—  Terminal  Index 8vo,     *2  50 

—  Lieber's  Appendix folio,  *i5  oo 

—  Handy  Tables 4to,     *2  50 

—  Bankers  and  Stockbrokers'  Code  and  Merchants  and  Shippers'  Blank 

Tables 8vo,  *is  oo 

—  100,000,000  Combination  Code 8vo,  *i$  oo 

—  Engineering  Code ,  , 8vo,  *io  oo 

kivermore,  V.  P.,  and  Williams,  J.     How  to  Become  a  Competent  Motor- 
man.  ,, , I2U10,      *I  QQ 


D.  VAN   NOSTRAND   COMPANY'S  SHORT  TITLE  CATALOG      15 

Livingstone,  R.     Design  and  Construction  of  Commutators 8vo,  *2  25 

Lobben,  P.     Machinists'  and  Draftsmen's  Handbook 8vo,  2  50 

Locke,  A.  G.  and  C.  G.     Manufacture  of  Sulphuric  Acid 8vo,  10  oo 

Lockwood,    T.     D.      Electricity,    Magnetism,      and     Electro-telegraph. 

8vo,  2  50 

—  Electrical  Measurement  and  the  Galvanometer i2mo,  i  50 

Lodge,  0.  J.     Elementary  Mechanics I2mo,  i  50 

—  Signalling  Across  Space  without  Wires 8vo,  *2  oo 

Lord,  R.  T.     Decorative  and  Fancy  Fabrics 8vo,  *3  50 

Loring,  A.  E.     A  Handbook  of  the  Electromagnetic  Telegraph i6mo,  o  50 

—  Handbook.     (Science  Series  No.  39.) i6mo,  o  50 

Lowenstein,  L.  C.,  and  Crissey,  C.  P.     Centrifugal  Pumps.  .  .  .  (In  Press.) 

Lucke,  C.  E.     Gas  Engine  Design 8vo,  *3  oo 

—  Power  Plants:  their  Design,  Efficiency,  and  Power  Costs.     2  vols. 

(In  Preparation.) 

—  Power  Plant  Papers.     Form  I.  The  Steam  Power  Plant paper,  *i  50 

Lunge,  G.     Coal-tar  and  Ammonia.     Two  Volumes 8vo,  *i$  oo 

—  Manufacture  of  Sulphuric  Acid  and  Alkali.     Three  Volumes ....  8vo, 

Vol.     I.     Sulphuric  Acid.     In  two  parts *i5  oo 

Vol.    II.     Salt  Cake,  Hydrochloric  Acid  and  Leblanc  Soda.      In  two 

parts *i5  oo 

Vol.  III.     Ammonia  Soda *I5  oo 

-  Technical  Chemists'  Handbook i2mo,  leather,  *3  50 

—  Technical  Methods  of  Chemical  Analysis.     Trans,  by  C.  A.  Keane. 

in  collaboration  with  the  corps  of  specialists. 

Vol.    I.     In  two  parts 8vo,  *i$  oo 

Vols.  II  and  III (In  Preparation.) 

Lupton,  A.,  Parr,  G.  D.  A.,  and  Perkin,  H.     Electricity  as  Applied  to 

Mining 8vo,  *4  50 

Luquer,  L.  M.     Minerals  in  Rock  Sections 8vo,  *i  50 

Macewen,  H.  A.     Food  Inspection .  .8vo,  *2  50 

Mackenzie,  N.  F.     Notes  on  Irrigation  Works 8vo,  *2  50 

Mackie,  J.     How  to  Make  a  Woolen  Mill  Pay .  .  8vo,  *2  oo 

Mackrow,  C.     Naval  Architect's  and  Shipbuilder's  Pocket-book. 

i6mo,  leather,  5  oo 

Maguire,  Capt.  E.     The  Attack  and  Defense  of  Coast  Fortifications.    .8vo,  2  50 

Maguire,  Wm.  R.     Domestic  Sanitary  Drainage  and  Plumbing 8vo,  4  oo 

Mallet,  A.     Compound  Engines.     Trans,  by  R.  R.  Buel.     (Science  Series 

No.  10.) i6mo, 

Mansfield,  A.  N.     Electro-magnets.     (Science  Series  No.  64.) . .      .  .  i6mo,  o  50 

Marks,  E.  C.  R.     Construction  of  Cranes  and  Lifting  Machinery i2mo,  *i  50 

—  Construction  and  Working  of  Pumps i2mo,  *i  50 

—  Manufacture  of  Iron  and  Steel  Tubes .  .  i2mo,  *2  oo 

Mechanical  Engineering  Materials I2mo,  *i  oo 


Marks,  G.  C.     Hydraulic  Power  Engineering 8vo,  3  50 

-  Inventions,  Patents  and  Designs I2mo,  *i  oo 

Markham,  E.  R.     The  American  Steel  Worker i2mo,  2  50 

Marlow,  T.  G.     Drying  Machinery  and  Practice .  .                                  .  .  8vo,  *5  oo 
Marsh,  C.  F.     Concise  Treatise  on  Reinforced  Concrete. ...                   8vo, 

Marsh,  C.  F.,  and  Dunn,  W*    Reinforced  Concrete .  .  4*o,  *5  oo 


16     D.  VAN  NOSTRAND  COMPANY'S  SHORT  TITLE  CATALOG 

Marsh,  C.  F.,  and  Dunn,  W.     Manual  of  Reinforced  Concrete  and  Con- 
crete Block  Construction i6mo,  morocco,  *2  50 

Massie,  W.  W.,  and  Underbill,  C.  R.     Wireless  Telegraphy  and  Telephony. 

i2mo,  *i  oo 
Matheson,  D.     Australian  Saw-Miller's  Log  and  Timber  Ready  Reckoner. 

i2mo,  leather,  i  50 

Mathot,  R.  E.     Internal  Combustion  Engines 8vo,  *6  oo 

Maurice,  W.     Electric  Blasting  Apparatus  and  Explosives 8vo,  *3  50 

—  Shot  Firer's  Guide 8vo,  *i  50 

Maxwell,  J.  C.     Matter  and  Motion.     (Science  Series  No.  36.) i6mo,  o  50 

Maxwell,  W.  H.,  and  Brown,  J.  T.     Encyclopedia  of  Municipal  and  Sani- 
tary Engineering 4to,  *io  oo 

Mayer,  A.  M.     Lecture  Notes  on  Physics 8vo,  2  oo 

McCullough,  R.  S.     Mechanical  Theory  of  Heat 8vo,  3  50 

Mclntosh,  J.  G.     Technology  of  Sugar 8vo,  *4  50 

—  Industrial  Alcohol 8vo,  *3  oo 

—  Manufacture  of  Varnishes  and  Kindred  Industries.     Three  Volumes. 

8vo. 

Vol.     I.     Oil  Crushing,  Refining  and  Boiling *3  50 

Vol.    II.     Varnish  Materials  and  Oil  Varnish  Making *4  oo 

Vol.  Ill (In  Preparation.) 

McKnight,  J.  D.,  and  Brown,  A.  W.     Marine  Multitubular  Boilers *i  50 

McMaster,  J.  B.     Bridge  and  Tunnel  Centres.     (Science  Series  No.  20.) 

i6mo,  o  50 

McMechen,  F.  L.     Tests  for  Ores,  Minerals  and  Metals i2mo,  *i  oo 

McNeill,  B.     McNeill's  Code 8vo,  *6  oo 

McPherson,  J.  A.     Water- works  Distribution 8vo,  2  50 

Melick,  C.  W.     Dairy  Laboratory  Guide i2mo,  *i  25 

Merck,  E.     Chemical  Reagents;  Their  Purity  and  Tests 8vo,  *i  50 

Merritt,  Wm.  H.     Field  Testing  for  Gold  and  Silver i6mo,  leather,  i  50 

Meyer,  J.  G.  A.,  and  Pecker,  C.  G.     Mechanical  Drawing  and  Machine 

Design 4to5  5  oo 

Michell,  S.     Mine  Drainage 8vo,  10  oo 

Mierzinski,  S.     Waterproofing  of  Fabrics.     Trans,  by  A.  Morris  and  H, 

Robson 8vo,  *2  50 

Miller,  E.  H.     Quantitative  Analysis  for  Mining  Engineers 8vo,  *i  50 

Miller,  G.  A.     Determinants.     (Science  Series  No.  105.) i6mo, 

Milroy,  M.  E.  W.     Home  Lace-m'aking i2mo,  *i  oo 

Minifie,  W.     Mechanical  Drawing 8vo,  *4  oo 

Mitchell,  C.  A.,  and  Prideaux,  R.  M.     Fibres  Used  in  Textile  and  Allied 

Industries 8vo, 

Modern  Meteorology i2mo,  i  50 

Monckton,  C.  C.  F.     Radiotelegraphy.     (Westminster  Series.) 8vo,  *2  op 

Monteverde,  R.  D.     Vest  Pocket  Glossary  of  English-Spanish,  Spanish- 
English  Technical  Terms 641110,  leather,  *i  oo 

Moore,  E.  C.  S.     New  Tables  for  the  Complete  Solution  of  Ganguillet  and 

Kutter's  Formula 8vo,  *5  oo 

Moreing,  C.  A.,  and  Neal,  T.    New  General  and  Mining  Telegraph  Code,  8vo,  *5  oo 

Morgan,  A.  P.     Wireless  Telegraph  Apparatus  for  Amateurs i2mo,  *i  50 

Moses,  A.  J.     The  Characters  of  Crystals 8vo,  *2  oo 

Moses,  A.  J.,  and  Parsons,  C.  L.     Elements  of  Mineralogy 8vo,  *2  SQ 


D.  VAN  NOSTRAND  COMPANY'S  SHORT  TITLE  CATALOG      17 

Moss,  S.  A.  Elements  of  Gas  Engine  Design.  (Science  Series  No.i2i.)i6mo,  o  50 

-  The  Lay-out  of  Corliss  Valve  Gears.    (Science  Series  No.  119.) .  i6mo,  o  50 

Mullin,  J.  P.     Modern  Moulding  and  Pattern-making i2mo,  2  50 

Munby,  A.  E.     Chemistry  and  Physics  of  Building  Materials.     (Westmin- 
ster Series.). .                                                                    8vo,  *2  oo 

Murphy,  J.  G.     Practical  Mining .    i6mo,  i  oo 

Murray,  J.  A.     Soils  and  Manures.     (Westminster  Series.) ..              .   8vo,  *2  oo 

Naquet,  A.     Legal  Chemistry .  .  i2mo,  2  oo 

Nasmith,  J.     The  Student's  Cotton  Spinning 8vo,  3  oo 

Neilson,  R.  M.     Aeroplane  Patents 8vo,  *2  oo 

Nerz,  F.     Searchlights.     Trans,  by  C.  Rodgers 8vo,  *3  oo 

Neuberger,  H.,  and  Noalhat,  H.     Technology  of  Petroleum.     Trans,  by  J. 

G.  Mclntosh 8vo,  *io  oo 

Newall,  J.  W.     Drawing,  Sizing  and  Cutting  Bevel-gears 8vo,  i  50 

Newlands,  J.     Carpenters  and  Joiners'  Assistant. folio,  half  morocco,  15  oo 

Nicol,  G.     Ship  Construction  and  Calculations 8vo,  *4  50 

Nipher,  F.  E.     Theory  of  Magnetic  Measurements I2mo,  i  oo 

Nisbet,  H.     Grammar  of  Textile  Design 8vo,  *3  oo 

Nolan,  H.     The  Telescope.     (Science  Series  No.  51.) i6mo,  o  50 

Noll,  A.     How  to  Wire  Buildings 12010,  i  50 

Nugent,  E.     Treatise  on  Optics i2mo,  i  50 

O'Connor,  H.     The  Gas  Engineer's  Pocketbook i2mo,  leather,  3  50 

—  Petrol  Air  Gas i2mo,  *o  75 

Ohm,   G.  S.,  and  Lockwood,  T.   D.     Galvanic   Circuit.     Translated  by 

William  Francis.  (Science  Series  No.  102.). i6mo,  o  50 

Olsson,  A.  Motor  Control,  in  Turret  Turning  and  Gun  Elevating.  (U.  S. 

Navy  Electrical  Series,  No.  i.). . .  .  i2mo,  paper,  *o  50 

Olsen,  J.  C.  Text-book  of  Quantitative  Chemical  Analysis. .  .  ,8vo,  *4  oo 

Oudin,  M.  A.  Standard  Polyphase  Apparatus  and  Systems . .  .  8vo,  *3  oo 

Palaz,  A.     Industrial  Photometry.     Trans,  by  G.  W.  Patterson,  Jr. .  .  8vo,  *4  oo 

Pamely,  C.     Colliery  Manager's  Handbook .8vo,  *io  oo 

Parr,  G.  D.  A.     Electrical  Engineering  Measuring  Instruments             8vo,  *3  50 

Parry,  E.  J.     Chemistry  of  Essential  Oils  and  Artificial  Perfumes         8vo,  *5  oo 

Parry,  E.  J.,  and  Coste.  J.  H.     Chemistry  of  Pigments                             8vo,  *4  50 

Parry,  L.  A.     Risk  and  Dangers  of  Various  Occupations. .                     8vo,  *3  oo 

Parshall,  H.  F.,  and  Hobart,  H.  M.     Armature  Windings                         4to,  *7  50 

-  Electric  Railway  Engineering.                                                            4*0,  *io  oo 
Parshall,  H.  F.,  and  Parry,  E.     Electrical  Equipment  of  Tramways. .  .  .  (In  P/r.s-.s.) 

Parsons,  S.  J.     Malleable  Cast  Iron 8vo,  *2  50 

Passmore,  A.  C.     Technical  Terms  Used  in  Architecture.                       8vo,  *3  50 

Patterson,  D.     The  Color  Printing  of  Carpet  Yarns.                              .8vo,  *3  50 

—  Color  Matching  on  Textiles 8vo,  *3  oo 

-  The  Science  of  Color  Mixing.  ...                                                     8vo,  *3  oo 
Patton,  H.  B.     Lecture  Notes  on  Crystallography. ..                              8vo,  *i  25 
Paulding,  C.  P.     Condensation  of  Steam  in  Covered  and  Bare  Pipes    8vo,  *2  oo 

-  Transmission  of  Heat  through  Cold-storage  Insulation.           .i2mo,  *i  oo 
Peirce,  B.     System  of  Analytic  Mechanics.                                              4*°»  10  oo 
Pendred,  V.     The  Railway  Locomotive.     (Westminster  Series.) ..       8vo,  *2  oo 
Perkin,  F.  M.     Practical  Methods  of  Inorganic  Chemistry.             .    i2mo,  *i  oo 


18     D.  VAN   NOSTRAND   COMPANY'S   SHORT   TITLE   CATALOG 

Perrigo,  0.  E.     Change  Gear  Devices 8vo,  i  oo 

Perrine,  F.  A.  C.     Conductors  for  Electrical  Distribution 8vo,  *3  50 

Petit,  G.     White  Lead  and  Zinc  White  Paints 8vo,  *i  50 

Petit,  R.     How  to  Build  an  Aeroplane.     Trans,  by  T.  O'B.  Hubbard,  and 

J.  H.  Ledeboer 8vo,  *i  50 

Pettit,  Lieut.  J.  S.     Graphic  Processes.     (Science  Series  No.  76.) .  .  .  i6mo,  o  50 

Perry,  J.     Applied  Mechanics 8vo,  *2  50 

Philbrick,  P.  H.     Beams  and  Girders.     (Science  Series  No.  88.) .  .  .  i6mo, 

Phillips,  J.     Engineering  Chemistry 8vo,  *4  50 

—  Gold  Assaying 8vo,  *2  50 

—  Dangerous  Goods 8vo,  3  50 

Phin,  J.     Seven  Follies  of  Science I2mo,  *i  25 

—  Household  Pests,  and  How  to  Get  Rid  of  Them 8vo  (In  Preparation.') 

Pickworth,  C.  N.     The  Indicator  Handbook.     Two  Volumes.  .  i2mo,  each,  i   50 

—  Logarithms  for  Beginners i2mo,  boards,  o  50 

—  The  Slide  Rule i2mo,  i  oo 

Plane  Table,  The 8vo,  2  oo 

Plattner's  Manual  of  Blow-pipe  Analysis.    Eighth  Edition,  revised.    Trans. 

by  H.  B.  Cornwall : 8vo,  *4  oo 

Plympton,  G.  W.    The  Aneroid  Barometer.    (Science  Series  No.  35.)    i6mo,  o  50 

—  How  to  become  an  Engineer.     (Science  Series  No.  100.) i6mo,  o  50 

—  Van  Nostrand's  Table  Book.     (Science  Series  No.  104.) i6mo,  o  50 

Pochet,  M.  L.     Steam  Injectors.     Translated  from  the  French.     (Science 

Series  No.  29.) i6mo,  o  50 

Pocket  Logarithms  to  Four  Places.     (Science  Series  No.  65.) i6mo,  o  50 

leather,  i  oo 

Pope,  F.  L.     Modern  Practice  of  the  Electric  Telegraph 8vo,  i  50 

Popple  well,  W.  C.  Elementary  Treatise  on  Heat  and  Heat  Engines.  .  i2mo,  *3  oo 

—  Prevention  of  Smoke 8vo,  *3  50 

—  Strength  of  Materials 8vo,  *i  75 

Potter,  T.     Concrete ». . . .  8vo,  *3  oo 

Practical  Compounding  of  Oils,  Tallow  and  Grease 8vo,  *3  50 

Practical  Iron  Founding I2mo,  i  50 

Pray,  T.,  Jr.     Twenty  Years  with  the  Indicator 8vo,  2  50 

—  Steam  Tables  and  Engine  Constant 8 vo,  2  oo 

—  Calorimeter  Tables  .  / 8vo,  i  oo 

Preece,  W.  H.     Electric  Lamps (In  Press.) 

Prelini,  C.     Earth  and  Rock  Excavation 8vo,  *3  oo 

—  Graphical  Determination  of  Earth  Slopes 8vo,  *2  oo 

—  Tunneling 8vo,  3  oo 

-  Dredging.     A  Practical  Treatise (In  Press.) 

Prescott,  A.  B.     Organic  Analysis 8vo,  5  oo 

Prescott,  A.  B.,  and  Johnson,  0.  C.     Qualitative  Chemical  Analysis.  .  .8vo,  *3  50 
Prescott,  A.  B.,  and  Sullivan,  E.  C.     First  Book  in  Qualitative  Chemistry. 

i2mo,  *i  50 

Pritchard,  O.  G.     The  Manufacture  of  Electric-light  Carbons .  .  8vo,  paper,  *o  60 
Prost,  E.     Chemical  Analysis  of  Fuels,  Ores,  Metals.     Trans,  by  J.  C. 

Smith 8vo,  *4  50 

Pullen,  W.  W.  F.     Application  of  Graphic  Methods  to  the  Design  of 

Structures i2mo,  *2  50 

—  Injectors;  Theory,  Construction  and  Working i2mo,  *i  50 


D.   VAN   NOSTRAND   COMPANY'S  SHORT  TITLE  CATALOG      19 

Pulsifer,  W.  H.     Notes  for  a  History  of  Lead 8vo,  4  oo 

Purchase,  W.  R.     Masonry iirao,  *3  oo 

Putsch,  A.     Gas  and  Coal-dust  Firing 8vo,  *3  oo 

Pynchon,  T.  R.     Introduction  to  Chemical  Physics 8vo,  3  oo 

Rafter  G.  W.     Mechanics  of  Ventilation.     (Science  Series  No.  33.) .  i6mo,  o  50 

—  Potable  Water.     (Science  Series  No.  103.) i6mo,  o  50 

-  Treatment  of  Septic  Sewage.     (Science  Series  No.  118.) i6mo,  o  50 

Rafter,  G.  W.,  and  Baker,  M.  N.     Sewage  Disposal  in  the  United  States  4to,  *6  oo 

Raikes,  H.  P.     Sewage  Disposal  Works   .                            8vo,  *4  oo 

Railway  Shop  Up-to-Date 4to,  2  oo 

Ramp,  H.  M.     Foundry  Practice (In  Press.) 

Randall,  P.  M.     Quartz  Operator's  Handbook.. i2mo,  2  oo 

Randau,  P.     Enamels  and  Enamelling 8vo,  *4  oo 

Rankine,  W.  J.  M.     Applied  Mechanics 8vo,  5  oo 

—  Civil  Engineering 8vo,  6  50 

—  Machinery  and  Millwork 8vo,  5  oo 

Rankine,  W.  J.  M.     The  Steam-engine  and  Other  Prime  Movers.    .  .   8vo,  5  oo 

—  Useful  Rules  and  Tables 8vo,  4  oo 

Rankine,  W.  J.  M.,  and  Bamber,  E.  F.     A  Mechanical  Text-book 8vo,  3  50 

Raphael,  F.  C.     Localization  of  Faults  in  Electric  Light  and  Power  Mains. 

8vo,  *3  oo 

Rathbone,  R.  L.  B.     Simple  Jewellery 8vo,  *2  oo 

Rateau,  A.     Flow  of  Steam  through  Nozzles  and  Orifices.     Trans,  bj  H. 

B.  Brydon 8vo,  *i  50 

Rausenberger,  F.     The  Theory  of  the  Recoil  of  Guns 8vo,  *4  50 

Rautenstrauch,  W.     Notes  on  the  Elements  of  Machine  Design,  8  vo,  boards,  *i  50 
Rautenstrauch,  W.,  and  Williams,  J.  T.     Machine  Drafting  and  Empirical 
Design. 

Part   I.  Machine  Drafting 8vo,  *i  25 

Part  II.  Empirical  Design (In  Preparation.) 

Raymond,  E.  B.     Alternating  Current  Engineering i2mo,  *2  50 

Rayner,  H.     Silk  Throwing  and  Waste  Silk  Spinning 8vo,  *2  50 

Recipes  for  the  Color,  Paint,  Varnish,  Oil,  Soap  and  Drysaltery  Trades  8vo,  *3  50 

Recipes  for  Flint  Glass  Making .  .  i2mo,  *4  50 

Redwood,  B.     Petroleum.     (Science  Series  No.  92.) i6mo,  o  50 

Reed's  Engineers'  Handbook 8vo,  *5  oo 

-  Key  to  the  Nineteenth  Edition  of  Reed's  Engineers'  Handbook .  .  8vo,  *3  oo 

—  Useful  Hints  to  Sea-going  Engineers i2mo,  i  50 

-  Marine  Boilers i2mo,  2  oo 

Reinhardt,  C.  W.     Lettering  for  Draftsmen,  Engineers,  and  Students. 

oblong  4to,  boards,  i  oo 

-  The  Technic  of  Mechanical  Drafting   .                  .  .  oblong  4to,  boards,  *i  oo 
Reiser,  F.     Hardening  and  Tempering  of  Steel.     Trans,  by  A.  Morris  and 

H.  Robson i2mo,  *2  50 

Reiser,  N.     Faults  in  the  Manufacture  of  Woolen  Goods.     Trans,  by  A. 

Morris  and  H.  Robson 8vo,  *2  50 

—  Spinning  and  Weaving  Calculations 8vo,  *5  oo 

Renwick,  W.  G.     Marble  and  Marble  Working. .                                    .8vo,  5  oo 
Reynolds,   0.,   and   Well,    F.   E.     Triple   Expansion   Engines.     (Science 

Series  No.  99.) l6mo»  °  So 


20     D    VAN   NOSTRAND   COMPANY'S  SHORT  TITLE  CATALOG 

Rhead,  G.  F.     Simple  Structural  Woodwork i2mo,  *i  oo 

Rice,  J.  M.,  and  Johnson,  W-  W.     A  New  Method  of  Obtaining  the  Differ- 
ential of  Functions i2mo,  o  50 

Richardson,  J.     The  Modern  Steam  Engine 8vo,  *3  50 

Richardson,  S.  S.     Magnetism  and  Electricity * i2mo,  *2  oo 

Rideal,  S.     Glue  and  Glue  Testing. 8vo,  *4  oo 

Rings,  F.     Concrete  in  Theory  and  Practice i2mo,  *2  50 

Ripper,  W.     Course  of  Instruction  in  Machine  Drawing folio,  *6  oo 

Roberts,  F.  C.     Figure  of  the  Earth.     (Science  Series  No.  79.) i6mo,  o  50 

Roberts,  J.,  Jr.     Laboratory  Work  in  Electrical  Engineering 8vo,  *2  oo 

Robertson,  L.  S.     Water-tube  Boilers 8vo,  3  oo 

Robinson,  J.  B.     Architectural  Composition 8vo,  *2  50 

Robinson,  S.  W.     Practical  Treatise  on  the  Teeth  of  Wheels.     (Science 

Series  No.  24.) .  .  . i6mo,  o  50 

—  Railroad  Economics.     (Science  Series  No.  59.) i6mo,  o  50 

-  Wrought  Iron  Bridge  Members.     (Science  Series  No.  60.) i6mo,  o  50 

Roebling,  J.  A.     Long  and  Short  Span  Railway  Bridges folio,  25  oo 

Rogers,  A.     A  Laboratory  Guide  of  Industrial  Chemistry i2mo,  *i  50 

Rogers,  A.,  and  Aubert,  A.  B.     Industrial  Chemistry (In  Press.) 

Rogers,  F.     Magnetism  of  Iron  Vessels.     (Science  Series  No.  30.) . .  i6mo,  o  50 

Rollins,  W.     Notes  on  X-Light 8vo,  *7  50 

Rose,  J.     The  Pattern-makers'  Assistant 8vo,  2  50 

—  Key  to  Engines  and  Engine-running I2mo,  2  50 

Rose,  T.  K.     The  Precious  Metals.     (Westminster  Series.) 8vo,  *2  oo 

Rosenhain,  W.     Glass  Manufacture.     (Westminster  Series.) 8vo,  *2  oo 

Ross,  W.  A.     Plowpipe  in  Chemistry  and  Metallurgy I2mo,  *2  oo 

Rossiter,  J.  T.     Steam  Engines.     (Westminster  Series.). .  .  .8vo  (In  Press.) 

— —  Pumps  and  Pumping  Machinery.     (Westminster  Series.).. 8vo  (In  Press.) 

Roth.     Physical  Chemistry 8vo,  *2  oo 

Rouillion,  L.     The  Economics  of  Manual  Training 8vo,  2  oo 

Rowan,  F.  J.     Practical  Physics  of  the  Modern  Steam-boiler 8vo,  7  50 

Rowan,   F.   J.,   and  Idell,   F.   E.     Boiler   Incrustation  and  Corrosion. 

(Science  Series  No.  27.) i6mo,  o  50 

Roxburgh,  Wo     General  Foundry  Practice 8vo,  *3  50 

Ruhmer,  E.     Wireless  Telephony.     Trans,  by  J.  Erskine-Murray ....  8vo,  *3  50 

Russell,  A.    Theory  of  Electric  Cables  and  Networks 8vo,  *3  oo 

Sabine,  R.     History  and  Progress  of  the  Electric  Telegraph i2mo,  i  25 

Saeltzer,  A.     Treatise  on  Acoustics i2mo,  i  oo 

Salomons,  D.     Electric  Light  Installations.     I2mo. 

Vol.    I.     The  Management  of  Accumulators 2  50 

Vol.  II.     Apparatus 2  25 

Vol.  III.     Applications i  50 

Sanford,  P.  G.     Nitro-explosives 8vo,  *4  oo 

Saunders,  C.  H.     Handbook  of  Practical  Mechanics i6rno,  i  oo 

leather,  i  25 

Saunnier,  C.     Watchmaker's  Handbook I2mo,  3  oo 

Sayers,  H.  M.     Brakes  for  Tram  Cars 8vo,  *i  25 

Scheele,  C.  W.     Chemical  Essays 8vo,  *2  oo 

Schellen,  H.     Magneto-electric  and  Dynamo-electric  Machines 8vo,  5  oo 

Scherer,  R.    Casein.     Trans,  by  C.  Salter .8vo,  *3  oo 


D.   VAN   NOSTRAND  COMPANY'S  SHORT  TITLE  CATALOG     21 

Schmall,  C.  N.     First  Course  in  Analytic  Geometry,  Plane  and  Solid. 

i2mo,  half  leather,  *i  75 

Schmall,  C.  N.,  and  Shack,  S.  M.     Elements  of  Plane  Geometry.  .  .    i2mo,  *i  25 

Schmeer,  L.     Flow  of  Water gvo,  *7  oo 

Schumann,  F.     A  Manual  of  Heating  and  Ventilation i2mo,  leather,  i  50 

Schwarz,  E.  H.  L.     Causal  Geology gvo,  *2  50 

Schweizer,  V.,  Distillation  of  Resins gvo,  *3  50 

Scott,  W.  W.     Qualitative  Analysis.     A  Laboratory  Manual 8vo,  *i  50 

Scribner,  J.  M.     Engineers'  and  Mechanics'  Companion  .  . .  i6mo,  leather,  i  50 
Searle,  G.  M.     "  Sumners'  Method."     Condensed  and  Improved.    (Science 

Series  No.  124.) i6mo,  o  50 

Seaton,  A.  E.     Manual  of  Marine  Engineering gvo,  6  oo 

Seaton,  A.  E.,  and  Rounthwaite,  H.  M.     Pocket-book  of  Marine  Engineer- 
ing  i6mo,  leather,  3  oo 

Seeligmann,  T.,  Torrilhon,  G.  L.,  and  Falconnet,  H.     India  Rubber  and 

Gutta  Percha.     Trans,  by  J.  G.  Mclntosh gvo,  *5  oo 

Seidell,  A.     Solubilities  of  Inorganic  and  Organic  Substances 8vo,  *3  oo 

Sellew,  W.  H.     Steel  Rails 4to  (In  Press.) 

Senter,  G.     Outlines  of  Physical  Chemistry i2mo,  *i  50 

Sever,  G.  F.     Electric  Engineering  Experiments 8vo,  boards,  *i  oo 

Sever,  G.  F.,  and  Townsend,  F.     Laboratory  and  Factory  Tests  in  Electrical 

Engineering 8vo,  *2  50 

Sewall,  C.  H.     Wireless  Telegraphy -. 8vo,  *2  oo 

—  Lessons  in  Telegraphy. I2mo,  *i  oo 

Sewell,  T.     Elements  of  Electrical  Engineering 8vo,  *3  oo 

-  The  Construction  of  Dynamos 8vo,  *3  oo 

Sexton,  A.  H.     Fuel  and  Refractory  Materials i2mo,  *2  50 

—  Chemistry  of  the  Materials  of  Engineering .I2mo,  *2  50 

—  Alloys  (Non- Ferrous) 8vo,  *3  oo 

-  The  Metallurgy  of  Iron  and  Steel 8vo,  *6  50 

Seymour,  A.     Practical  Lithography 8vo,  *2  50 

—  Modern  Printing  Inks 8vo,  *2  oo 

Shaw,  Henry  S.  H.     Mechanical  Integrators.     (Science  Series  No.  83.) 

i6mo,  o  50 

Shaw,  P.  E.     Course  of  Practical  Magnetism  and  Electricity 8vo,  *i  oo 

Shaw,  S.     History  of  the  Staffordshire  Potteries ....                           .  .  8vo,  *3  oo 

—  Chemistry  of  Compounds  Used  in  Porcelain  Manufacture 8vo,  *s  oo 

Sheldon,  S.,  and  Hausmann,  E.     Direct  Current  Machines 8vo,  *2  50 

Sheldon,  S.,  Mason,  H.,  and  Hausmann,  E.     Alternating-current  Machines. 

8vo,  *2  50 

Sherer,  R.  Casein.  Trans,  by  C.  Salter .  -8vo,  *3  oo 

Sherriff,  F.  F.  Oil  Merchants'  Manual. .  .  -  i2mo,  ^3  50 

Shields,  J.  E.  Notes  on  Engineering  Construction .  .  i2mo,  i  50 

Shock,  W.  H.  Steam  Boilers .  -4to,  half  morocco,  15  oo 

Shreve,  S.  H.  Strength  of  Bridges  and  Roofs. .  8vo,  350 

Shunk,  W.  F.  The  Field  Engineer .  .  i2mo,  morocco,  2  50 

Simmons,  W.  H.,  and  Appleton,  H.  A.  Handbook  of  Soap  Manufacture. 

8vo,  *3  oo 

Simms,  F.  W.  The  Principles  and  Practice  of  Leveling.  .  .8vo,  2  oo 

-  Practical  Tunneling 8vo,  7  50 

Simpson,  G.    The  Naval  Constructor. . .                           •  •  I2mo,  morocco,  *5  50 


22     D.  VAN  NOSTRAND  COMPANY'S  SHORT  TITLE  CATALOG 

Sinclair,  A.     Development  of  the  Locomotive  Engine  .  . .  8vo,  half  leather,  5  oo 

Sindall,  R.  W.     Manufacture  of  Paper.     (Westminster  Series.) 8vo,  *2  oo 

Sloane,  T.  O'C.     Elementary  Electrical  Calculations i2mo,  *2  oo 

Smith,  C.  F.     Practical  Alternating  Currents  and  Testing 8vo,  *2  50 

—  Practical  Testing  of  Dynamos  and  Motors 8vo,  *2  oo 

Smith,  F.  E.     Handbook  of  General  Instruction  for  Mechanics.  .  .  .  i2mo,  i  50 
Smith,  I.  W.     The  Theory  of  Deflections  and  of  Latitudes  and  Departures. 

i6mo,  morocco,  3  oo 

Smith,  J.  C.     Manufacture  of  Paint 8vo,  *3  oo 

Smith,  W.     Chemistry  of  Hat  Manufacturing I2mo,  *3  oo 

Snell,  A.  T.     Electric  Motive  Power 8vo,  *4  oo 

Snow,  W.  G.     Pocketbook  of  Steam  Heating  and  Ventilation.    (In  Press.) 
Snow,  W.  G.,  and  Nolan,  T.     Ventilation  of  Buildings.     (Science  Series 

No.  5.) i6mo,  o  50 

Soddy,  F.     Radioactivity 8vo,  *3  oo 

Solomon,  M.     Electric  Lamps.     (Westminster  Series.) 8vo,  *2  oo 

Sothern,  J.  W.     The  Marine  Steam  Turbine 8vo,  *s  oo 

Soxhlet,  D.  H.     Dyeing  and  Staining  Marble.     Trans,  by  A.  Morris  and 

H.  Robson 8vo,  *2  50 

Spang,  H  .W.     A  Practical  Treatise  on  Lightning  Protection i2mo,  i  oo 

Spangenburg,    L.     Fatigue    of    Metals.     Translated    by    S.    H.    Shreve. 

(Science  Series  No.  23.) i6mo,  o  50 

Specht,  G.  J.,  Hardy,  A.  S.,  McMaster,  J.  B.,  and  Walling.     Topographical 

Surveying.     (Science  Series  No.  72.) i6mo,  o  50 

Speyers,  C.  L.     Text-book  of  Physical  Chemistry 8vo,  *2  25 

Stahl,  A.  W.     Transmission  of  Power.     (Science  Series  No.  28.) . .  .  i6mo, 

Stahl,  A.  W.,  and  Woods,  A.  T.     Elementary  Mechanism I2mo,  *2  oo 

Staley,  C.,  and  Pierson,  G.  S.     The  Separate  System  of  Sewerage.  .  .  .8vo,  *3  oo 

Standage,  H.  C.     Leatherworkers'  Manual 8vo,  *3  50 

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Stansbie,  J.  H.     Iron  and  Steel.     (Westminster  Series.) 8vo,  *2  oo 

Stevens,  H.  P.     Paper  Mill  Chemist i6mo,  *2  50 

Stevenson,  J.  L.     Blast-Furnace  Calculations i2mo,  leather,  *2  oo 

Stewart,  A.     Modern  Polyphase  Machinery i2mo,  *2  oo 

Stewart,  G.     Modern  Steam  Traps i2mo,  *i  25 

Stiles,  A.     Tables  for  Field  Engineers i2mo,  i  oo 

Stillman,  P.     Steam-engine  Indicator i2mo,  i  oo 

Stodola,  A.     Steam  Turbines.     Trans,  by  L.  C.  Loewenstein 8vo,  *s  oo 

Stone,  H.     The  Timbers  of  Commerce 8vo,  3  50 

Stone,  Gen.  R.    New  Roads  and  Road  Laws i2mo,  i  oo 

Stopes,  M.     Ancient  Plants 8vo,  *2  oo 

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Suffling,  E.  R.     Treatise  on  the  Art  of  Glass  Painting 8vo,  *3  50 

Swan,  K.     Patents,   Designs  and   Trade   Marks.      { Westminster   Series.) 

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Sweet,  S.  H.     Special  Report  on  Coal 8vo,  3  oo 

Swinburne,  J.,  Wordingham,  C.  H.,  and  Martin,  T.  C.     Eletcric  Currents. 

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Tate,  J.  S.     Surcharged  and  Different  Forms  of  Retaining-walls.     (Science 
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Templeton,  W.     Practical  Mechanic's  Workshop  Companion. 

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Terry,  H.  L.     India  Rubber  and  its  Manufacture.     (Westminster  Series.) 

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Thorn,  C.,  and  Jones,  W.  H      Telegraphic  Connections          oblong  i2mo,  i  50 
Thomas,  C.  W.     Paper-makers'  Handbook  ......                      .  .(In  /V.s.x.) 

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Thompson,  E.  P.     How  to  Make  Indentions  .......................  8vo,  o  50 

Thompson,  S.  P.     Dynamo  Electric  Machines.     (Science  Series  No.  75.) 

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Thompson,  W.  P.     Handbook  of  Patent  Law  of  All  Countries  ......  i6mo,  i  50 

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Tidy,  C.  Meymott.     Treatment  of  Sewage.     (Science  Series  No.  94.).  i6mo,  o  50 

Tinney,  W.  H.     Gold-mining  Machinery  .........................  8vo,  *s  oo 

Titherley,  A.  W.     Laboratory  Course  of  Organic  Chemistry  .........  8vo,  *2  oo 

Toch,  M.     Chemistry  and  Technology  of  Mixed  Paints  ..............  8vo,  *3  oo 

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Todd,  J.,  and  Whall,  W.  B.     Practical  Seamanship.  .                          .  .8vo,  *7  50 

Tonge,  J.     Coal.     (Westminster  Series.)  ..........                              .  .  8vo,  *2  oo 

Townsend,  F.     Alternating  Current  Engineering  ........  8vo,  boards  *o  75 

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Trowbridge,  W.  P.     Turbine  Wheels.     (Science  Series  No.  44-)--   .-i6mo,  o  50 

Tucker,  J.  H.     A  Manual  of  Sugar  Analysis.  .                                          8vo,  3  50 

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Turnbull,  Jr.,  J.,  and  Robinson,  S.  W.     A  Treatise  on  the  Compound 
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Turrill,  S.  M.     Elementary  Course  in  Perspective.  .                              i2mo,  *i  25 

Underbill,  C.  R.     Solenoids,  Electromagnets  and  Electromagnetic  Wind- 

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Urquhart,  J.  W.     Electric  Light  Fitting  ........  •    "mo. 

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24     D.  VAN   NOSTRAND   COMPANY'S   SHORT  TTTLK    CATALOG 

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Vacher,  F.  Food  Inspector's  Handbook i2mo,  *2  50 

Van  Nostrand's  Chemical  Annual.  Second  issue  1909 i2mo,  *2  50 

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Van  Wagenen,  T.  F.  Manual  of  Hydraulic  Mining i6mo,  i  oo 

Vega,  Baron  Von.  Logarithmic  Tables 8vo,  half  morocco,  2  50 

Villon,  A.  M.  Practical  Treatise  on  the  Leather  Industry.  Trans,  by  F. 

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Vincent,  C.  Ammonia  and  its  Compounds.  Trans,  by  M.  J.  Salter.  .8vo,  *2  oo 

Volk,  C.  Haulage  and  Winding  Appliances 8vo,  *4  oo 

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Vose,  G.  L.     Graphic  Method  for  Solving  Certain  Questions  in  Arithmetic 

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Wabner,  R.     Ventilation  in  Mines.     Trans,  by  C.  Salter . .  ., 8vo,  *4  50 

Wade,  E.  J.     Secondary  Batteries 8vo,  *4  oo 

Wadsworth,  C.     Primary  Battery  Ignition i2mo  (In  Prc.s.s.) 

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Walker,  F.     Aerial  Navigation 8vo,  2  oo 

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Walker,  S.  F.     Steam  Boilers,  Engines  and  Turbines 8vo,  3  oo 

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Wanklyn,  J.  A.     Treatise  on  the  Examination  of  Milk i2mo,  i  oo 

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Weather  and  Weather  Instruments I2mo,  i  oo 

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Webb,  H.  L.     Guide  to  the  Testing  of  Insulated  Wires  and  Cables. .  i2mo,  i  oo 

Webber,  W.  H.  Y.     Town  Gas.     (Westminster  Series.) 8vo,  *2  oo 

Weekes,  R.  W.     The  Design  of  Alternate  Current  Transformers i2mo,  i  oo 

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Weisbach,  J.,  and  Herrmann,  G.     Mechanics  of  Air  Machinery 8vo,  *3  75 

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Wheeler,  J.  B.     Art  of  War I2mo,  i  75 

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Whipple,  S.     An  Elementary  and  Practical  Treatise  on  Bridge  Building. 

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Whithard,  P.     Illuminating  and  Missal  Painting i2mo,  i  50 

Wilcox,  R.  M.     Cantilever  Bridges.     (Science  Series  No.  25.) i6mo,  o  50 

Wilkinson,  H.  D.     Submarine  Cable  Laying  and  Repairing 8vo,  *6  oo 

Williams,  A.  D.,  Jr.,  and  Hutchinson,  R.  W.     The  Steam  Turbine (In  Press.) 

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Wisser,  Lieut.  J.  P.     Explosive  Materials.     (Science  Series  No.  70.) 

i6mo,  o  50 

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Wood,  De  V.     Luminiferous  Aether.     (Science  Series  No.  85.) i6mo,  o  50 

Woodbury,  D.  V.     Elements  of  Stability  in  the  Well-proportioned  Arch. 

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Wright,  T.  W.     Elements  of  Mechanics 8vo,  *2  50 

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26     D.   VAN   NOSTRAND    COMPANY'S   SHORT   TITLE  CATALOG 

Zahner,  R.     Transmission  of  Power.     (Science  Series  No.  40..) ....  i6mo, 

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Zipser,  J.     Textile  Raw  Materials.     Trans,  by  C.  Salter 8vo,     *5  oo 

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